Answer:
Answer in explanation
Explanation:
a. Carbon, atomic number 6
Helium has 2 electrons. We add this to the other 4 to make 6
Other group elements: Silicon Si, Germanium Ge , Tin Sn , lead Pb , Flerovium Fl
b. Vanadium, atomic number 23
Argon has 18 electrons, we add 5 to the 18 to make 23
Other group members are: Niobium Nb, Tantalum Ta , Dubnium Db
c. Phosphorus, atomic number 15
Neon has atomic number of 10
Other group members are: Nitrogen N , Phosphorus P , Arsenic As , Antimony Sb , Bismuth Bi and Moscovium Mc
A 4.00 gram sample of a solution of sodium chloride in water was heated until all the water had evaporated. The sodium chloride that remained weighed 1.22 grams. Calculate the percentage of water in the original 4.00 grams of solution.
The weight of the water in the original solution is 2.78 grams. The percentage of water in the original 4.00 grams solution of sodium chloride, once the water was evaporated, is therefore approximately 69.5%.
Explanation:The weight of the water in the original solution can be found by subtracting the weight of the remaining sodium chloride from the total weight of the solution. So, water = total weight - weight of sodium chloride = 4.00 grams - 1.22 grams = 2.78 grams.
The percentage of water in the solution can be found by the following formula:
Percentage = (Weight of water / Total weight) * 100 = (2.78 grams / 4.00 grams) * 100 = 69.5%
So, the percentage of water in the 4.00 gram solution of sodium chloride after the water was evaporated, is approximately 69.5%.
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Name the element described in each of the following:
(a) Smallest atomic radius in Group 6A(16)
(b) Largest atomic radius in Period 6
(c) Smallest metal in Period 3
(d) Highest IE₁ in Group 4A(14)
(e) Lowest IE₁ in Period 5
(f) Most metallic in Group 5A(15)
(g) Group 3A(13) element that forms the most basic oxide
(h) Period 4 element with filled outer level
(i) Condensed ground-state electron configuration of [Ne] 3s²3p²
(j) Condensed ground-state electron configuration of [Kr] 5s²4d⁶
(k) Forms 2+ ion with electron configuration [Ar] 3d³
(l) Period 5 element that forms 3+ ion with pseudo–noble gas configuration
(m) Period 4 transition element that forms 3+ diamagnetic ion
(n) Period 4 transition element that forms 2+ ion with a halffilled d sublevel
(o) Heaviest lanthanide
(p) Period 3 element whose 2- ion is isoelectronic with Ar
(q) Alkaline earth metal whose cation is isoelectronic with Kr
(r) Group 5A(15) metalloid with the most acidic oxide
Answer:
a. Smallest atomic radius in 6A – Oxygen (O)
b. Largest atomic radius in Period 6 – Cesium (Cs)
c. Smallest metal in period 3 – Aluminum (Al)
d. Highest IE1 in Group 4A –Carbon (C)
e. Lowest IE1 in period 5 – Rubidium (Rb)
f. Most metallic in Group 5A – Bismuth (Bi) or element 115
g. Group 3A element that forms the most basic oxide – Thallium
(Tl) or element 113
h. Period 4 element with filled outer level – Krypton (Kr)
i. Condensed gound state configuration is [Ne]3s23p2 –
Germanium (Ge)
j. Condensed ground state configuration is [Kr]5s24d6 –
Ruthenium (Ru)
k. Forms 2+ ion with electron configuration of [Ar]3d3 – Vanadium
(V)
l. Period 5 element that forms 3+ ion with pseudo‐noble gas
configuration – Indium (In)
m. Period 4 transition element that forms 3+ diamagnetic ion –
Scandium (Sc)
n. Period 4 transition element that forms 2+ ion with half‐filled d
sublevel – Manganese (Mn)
o. Heaviest Lanthanide – Lutetium (Lu)
p. Period 3 element whose 2‐ ion is isoelectronic with Ar – Sulfur
(S)
q. Alkali earth metal whose cation is isoelectronic with Kr –
Strontium (Sr)
r. Group 5 A metalloid with the most acidic oxide – Arsenic (As) or
Antimony (Sb)
Elements in a group are chemically similar to each other.
The periodic table is an arrangement of elements in groups and periods. The elements in the same group share a lot of chemical similarity with each other. The elements that are in the same period only have the same number of valence shells.
The elements described by each statement is;
(a) Smallest atomic radius in Group 6A(16) - oxygen
(b) Largest atomic radius in Period 6 - cesium
(c) Smallest metal in Period 3 - Aluminium
(d) Highest IE₁ in Group 4A(14) - carbon
(e) Lowest IE₁ in Period 5 - Bismuth
(g) Group 3A(13) element that forms the most basic oxide - Thallium
(h) Period 4 element with filled outer level - krypton
(i) Condensed ground-state electron configuration of [Ne] 3s²3p² - silicon
(j) Condensed ground-state electron configuration of [Kr] 5s²4d⁶- xenon
(k) Forms 2+ ion with electron configuration [Ar] 3d³ - vanadium
(l) Period 5 element that forms 3+ ion with pseudo–noble gas configuration - Indium
(m) Period 4 transition element that forms 3+ diamagnetic ion - Scandium
(n) Period 4 transition element that forms 2+ ion with a halffilled d sublevel - Manganese
(o) Heaviest lanthanide - Lutetium
(p) Period 3 element whose 2- ion is isoelectronic with Ar - sulfur
(q) Alkaline earth metal whose cation is isoelectronic with Kr - Strontium
(r) Group 5A(15) metalloid with the most acidic oxide - nitrogen
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Two moles of nitrogen are initially at 10 bar and 600 K (state 1) in a horizontal piston/cylinder device. They are expanded adiabatically to 1 bar (state 2). They are then heated at constant volume to 600 K (state 3). Finally, they are isothermally returned to state 1. Assume that N 2 is an ideal gas with a constant heat capacity as given on the back flap of the book. Neglect the heat capacity of the piston/cylinder device. Suppose that heat can be supplied or rejected as illustrated below. Assume each step of the process is reversible. Calculate the net work done overall.
Answer:
Net work done overall = sum of work done for all the processes = 16,995.84 J
Explanation:
From the start, P₁ = 10bar = 1 × 10⁶ Pa, T₁ = 600K, V₁ = ?
We can obtain V from PV = nRT; n = 2, R = 8.314 J/mol.K
V = 2 × 8.314 × 600/(1000000) = 0.009977 m³
P₁ = 10bar = 1 × 10⁶ Pa, T₁ = 600K, V₁ = 0.009977 m³
For an adiabatic process for an ideal gas,
P(V^γ) = constant
γ = ratio of specific heats = Cp/CV = 1.4,
P₂ = 1 bar = 10⁵ Pa
P₁ (V₁^1.4) = P₂ (V₂^1.4) = k
10⁶ (0.009977^1.4) = 10⁵(V₂^1.4) = 1579.75 = k
V₂ = 0.0517 m³
Work done for an adiabatic process
W = k((V₂^(1-γ)) - (V₁^(1-γ))/(1-γ)
W = 1579.75 ((0.0517^0.4) - (0.009977^0.4))/0.4
W = 582.25 J
We still need T₂
PV = nRT
T₂ = P₂V₂/nR = 100000×0.0517/(2×8.314) = 310.92K
Step 2, constant volume heating,
Work done at constant volume is 0 J.
T₂ = 310.92K, T₃ = 600K
V₂ = 0.0517 m³, V₃ = V₂ = 0.0517 m³ (Constant volume)
P₂ = 1bar, P₃ = ?
PV = nRT
P₃ = nRT₃/V₃ = 2 × 8.314 × 600/0.0517 = 192974.85 Pa = 1.93bar
Step 3, isothermally returned to the initial state.
P₃ = 1.93bar, P₄ = P₁ = 10bar
T₃ = 600K, T₄ = T₁ = 600K (Isothermal process)
V₃ = 0.0517 m³, V₄ = V₁ = 0.009977 m³
Work done = nRT In (V₃/V₁) = 2 × 8.314 × 600 In (0.0517/0.009977) = 16413.59 J
Net work done = W₁₂ + W₂₃ + W₃₁ = 582.25 + 0 + 16413.59 = 16995.84 J
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g Nitrogen in the atmosphere consists of two nitrogen atoms covalently bonded together (N2). Knowing that nitrogen is atomic number 7, what type of covalent bond holds those two atoms together?
Explanation:
Since, the atomic number of nitrogen is 7 and its electronic distribution is 2, 5. So, in order to attain stability it needs to gain 3 electrons.
Hence, when it chemically combines another nitrogen atom then as both the atoms are non-metals. So, sharing of electrons will take place.
Also, there is no difference in electronegativity of two nitrogen atoms. Hence, compound formed [tex]N_{2}[/tex] is non-polar covalent in nature.
Answer:
non polar bond
Explanation:
Consider a gas mixture in a 2.00-dm3 flask at 27.0 ºC. For each of the following mixtures, calculate the partial pressure of each gas, the total pressure, and the composition of the mixture in mole percent. a) 1.00 g H2 and 1.00 g O2 b) 1.00 g N2 and 1.00 g O2 c) 1.00 g CH4 and 1.00 g NH3
Explanation:
a)
Moles of hydrogen gas = [tex]n_1=\frac{1.00 g}{2 g/mol}=0.5 mol[/tex]
Moles of oxygen gas = [tex]n_2=\frac{1.00 g}{32 g/mol}=0.03125 mol[/tex]
Total moles in container = [tex]n=n_1+n_2=0.5 mol+0.03125 mol=0.53125 mol[/tex]
Total pressure of mixture = P
Temperature of the mixture = [tex]T = 27^oC =27+273K= 300 K[/tex]
Volume of the container in which mixture is kept = [tex]2.00 dm^3 =2.00 L[/tex]
[tex]1 dm^3=1 L[/tex]
[tex]P=\frac{nRT}{V}[/tex] (from ideal gas equation )
[tex]P=\frac{0.53125 mol\times 0.0821 atm L/mol K\times 300 K}{2.00 L}=6.54 atm[/tex]
Partial pressure of the hydrogen gas :
= [tex]p_1=P\times \chi_1=P\times \frac{n_1}{n}[/tex]
[tex]=6.54 atm\times \frac{0.5 mol}{0.53125 mol}=6.16 atm[/tex]
Partial pressure of the oxygen gas :
= [tex]p_2=P\times \chi_2=P\times \frac{n_2}{n}[/tex]
[tex]=6.54 atm\times \frac{0.03125 mol}{0.53125 mol}=0.38 atm[/tex]
hydrogen
= [tex]\frac{n_1}{n}\times 100=\frac{0.5 mol}{0.53125 }\times 100[/tex]
= 94.12%
oxygen :
= [tex]\frac{n_2}{n}\times 100=\frac{0.03125 mol}{0.53125 mol}\times 100[/tex]
= 5.88%
b)
Moles of nitrogen gas = [tex]n_1=\frac{1.00 g}{28 g/mol}=0.03571 mol[/tex]
Moles of oxygen gas = [tex]n_2=\frac{1.00 g}{32 g/mol}=0.03125 mol[/tex]
Total moles in container = [tex]n=n_1+n_2=0.03571 mol+0.03125 mol=0.06696 mol[/tex]
Total pressure of mixture = P
Temperature of the mixture = [tex]T = 27^oC =27+273K= 300 K[/tex]
Volume of the container in which mixture is kept = [tex]2.00 dm^3 =2.00 L[/tex]
[tex]1 dm^3=1 L[/tex]
[tex]P=\frac{nRT}{V}[/tex] (from ideal gas equation )
[tex]P=\frac{0.06696 mol\times 0.0821 atm L/mol K\times 300 K}{2.00 L}=0.82 atm[/tex]
Partial pressure of the nitrogen gas :
= [tex]p_1=P\times \chi_1=P\times \frac{n_1}{n}[/tex]
[tex]=0.82 atm\times \frac{0.03571 mol}{0.06696 mol}=0.44 atm[/tex]
Partial pressure of the oxygen gas :
= [tex]p_2=P\times \chi_2=P\times \frac{n_2}{n}[/tex]
[tex]=0.82 atm\times \frac{0.03125 mol}{0.06696 mol}=0.38 atm[/tex]
Composition of each in mole percent :
nitrogen
= [tex]\frac{n_1}{n}\times 100=\frac{0.03571 mol}{0.06696 }\times 100[/tex]
= 53.33%
oxygen :
= [tex]\frac{n_2}{n}\times 100=\frac{0.03125 mol}{0.06696 mol}\times 100[/tex]
= 46.67%
c)
Moles of methane gas = [tex]n_1=\frac{1.00 g}{16 g/mol}=0.0625 mol[/tex]
Moles of ammonia gas = [tex]n_2=\frac{1.00 g}{17g/mol}=0.0588 mol[/tex]
Total moles in container = [tex]n=n_1+n_2=0.0625 mol+0.0588 mol=0.1213 mol[/tex]
Total pressure of mixture = P
Temperature of the mixture = [tex]T = 27^oC =27+273K= 300 K[/tex]
Volume of the container in which mixture is kept = [tex]2.00 dm^3 =2.00 L[/tex]
[tex]1 dm^3=1 L[/tex]
[tex]P=\frac{nRT}{V}[/tex] (from ideal gas equation )
[tex]P=\frac{0.1213 mol\times 0.0821 atm L/mol K\times 300 K}{2.00 L}=1.49 atm[/tex]
Partial pressure of the methane gas :
= [tex]p_1=P\times \chi_1=P\times \frac{n_1}{n}[/tex]
[tex]=1.49 atm\times \frac{0.0625 mol}{0.1213mol}=0.77 atm[/tex]
Partial pressure of the ammonia gas :
= [tex]p_2=P\times \chi_2=P\times \frac{n_2}{n}[/tex]
[tex]=1.49 atm\times \frac{0.0588 mol}{0.1213mol}=0.72 atm[/tex]
Composition of each in mole percent :
Methane :
= [tex]\frac{n_1}{n}\times 100=\frac{0.0625 mol}{0.1213mol}\times 100[/tex]
= 51.52%
Ammonia
= [tex]\frac{n_2}{n}\times 100=\frac{0.0588 mol}{0.1213mol}\times 100[/tex]
= 48.47%
To calculate the partial pressure of each gas and the composition of the mixture, we can use the ideal gas law. By dividing the mass of each gas by its molar mass, we can calculate the number of moles. The total pressure can be obtained by summing up the partial pressures, and the mole percent composition can be calculated by dividing the number of moles of each gas by the total number of moles and multiplying by 100.
Explanation:To calculate the partial pressure of each gas, we need to use the ideal gas law. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. To calculate the total pressure, we can sum up the partial pressures of each gas. The mole percent composition can be calculated by dividing the number of moles of each gas by the total number of moles and multiplying by 100.
a) 1.00 g H2 and 1.00 g O2:
To calculate the number of moles, we divide the mass of each gas by its molar mass. The molar mass of H2 is 2 g/mol and the molar mass of O2 is 32 g/mol. So, the number of moles of H2 is 1 g / 2 g/mol = 0.5 mol, and the number of moles of O2 is 1 g / 32 g/mol = 0.03125 mol. The total number of moles is 0.5 mol + 0.03125 mol = 0.53125 mol.
The partial pressure of H2 can be calculated by multiplying the number of moles of H2 by the gas constant R and the temperature in Kelvin, and then dividing by the volume. The same process can be applied to calculate the partial pressure of O2. Finally, the total pressure can be calculated by summing up the partial pressures. The mole percent composition can be calculated by dividing the number of moles of each gas by the total number of moles and multiplying by 100.
b) 1.00 g N2 and 1.00 g O2:
Using the same process as before, we can calculate the number of moles of N2 and O2. The molar mass of N2 is 28 g/mol, so 1 g of N2 is equal to 1 g / 28 g/mol = 0.03571 mol of N2. The molar mass of O2 is 32 g/mol, so 1 g of O2 is equal to 1 g / 32 g/mol = 0.03125 mol of O2. The total number of moles is 0.03571 mol + 0.03125 mol = 0.06696 mol.
Using the ideal gas law, we can calculate the partial pressures of N2 and O2, the total pressure, and the mole percent composition.
c) 1.00 g CH4 and 1.00 g NH3:
Following the same calculations as above, the molar mass of CH4 is 16 g/mol, so 1 g of CH4 is equal to 1 g / 16 g/mol = 0.0625 mol of CH4. The molar mass of NH3 is 17 g/mol, so 1 g of NH3 is equal to 1 g / 17 g/mol = 0.05882 mol of NH3. The total number of moles is 0.0625 mol + 0.05882 mol = 0.12132 mol.
By using the ideal gas law, we can calculate the partial pressures of CH4 and NH3, the total pressure, and the mole percent composition.
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Which contains the greatest mass of oxygen: 0.75 moles of ethanol ( C2H5OH ), 0.60 mole of formic acid ( HCO2H ), or 1.0 mole of water ( H2O )? Why?
Answer:
0.60 mole of formic acid contains the greatest mass of oxygen
(19.2 grams)
Explanation:
Step 1: Data given
Moles of ethanol = 0.75 moles
Molar mass ethanol = 46.07 g/mol
Moles of formic acid = 0.60 moles
Molar mass of formic acid = 46.03 g/mol
Moles of H2O = 1.0
Molar mass of H2O = 18.02 g/mol
Step 2: Calculate moles of oxygen in each
Ethanol: For 1 mol ethanol we have 1 mol oxygen
For 0.75 moles ethanol we have 0.75 moles O
Mass O = 0.75 moles * 16.0 g/mol = 12.0 grams O
Formic acid: For 1 mol formic acid, we have 2 moles O
For 0.60 moles formic acid, we have 2*0.60 = 1.20 moles O
Mass O = 1.20 moles * 16.0 g/mol = 19.2 grams O
H2O: for 1.0 mol H2O we have 1 mol O
Mass O = 18.02 g/mol * 1.0 mol = 18.02 grams
0.60 mole of formic acid contains the greatest mass of oxygen
(19.2 grams)
Formic acid (HCO₂H) contains the greatest mass of oxygen among the three compounds with 19.2 grams of oxygen.
Step 1: Molar Mass of Oxygen
The molar mass of oxygen (O) is approximately 16 grams per mole (g/mol).
Step 2: Identify the Number of Oxygen Atoms in Each Compound
Ethanol (C₂H₅OH) has 1 oxygen atom.Formic acid (HCO₂H) also has 2 oxygen atoms.Water (H₂O) has 1 oxygen atom.Step 3: Calculate the Mass of Oxygen in Each Compound
Ethanol (C₂H₅OH):
Moles of oxygen = 0.75 moles of C₂H₅OH × 1 O atom/mole = 0.75 moles of O. Mass of oxygen = 0.75 moles × 16 g/mol = 12 g.Formic Acid (HCO₂H):
Moles of oxygen = 0.60 moles of HCO₂H × 2 O atoms/mole = 1.20 moles of O. Mass of oxygen = 1.20 moles × 16 g/mol = 19.2 g.Water (H₂O):
Moles of oxygen = 1.0 mole of H₂O × 1 O atom/mole = 1.0 mole of O. Mass of oxygen = 1.0 mole × 16 g/mol = 16 g.Step 4: Compare the Masses of Oxygen
Ethanol: 12 g Formic Acid: 19.2 g Water: 16 gExpress your answer as a balanced chemical equation. Identify all of the phases in your answer.
1. Li(s)+N2(g)→Li3N(s)
2. TiCl4(l)+H2O(l)→TiO2(s)+HCl(aq)
3. NH4NO3(s)→N2(g)+O2(g)+H2O(g)
4. Ca3P2(s)+H2O(l)→Ca(OH)2(aq)+PH3(g)
5. Al(OH)3(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2O(l)
6.AgNO3(aq)+Na2SO4(aq)→Ag2SO4(s)+NaNO3(aq)
7. C2H5NH2(g)+O2(g)→CO2(g)+H2O(g)+N2(g)
Explanation:
Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.
This also means that total mass on the reactant side must be equal to the total mass on the product side.
1.[tex]Li(s)+N_2(g)\rightarrow Li_3N(s)[/tex]
The balanced equation is:
[tex]6Li(s)+N_2(g)\rightarrow 2Li_3N(s)[/tex]
2. [tex]TiCl_4(l)+H_2O(l)\rightarrow TiO_2(s)+HCl(aq)[/tex]
The balanced equation is:
[tex]TiCl_4(l)+2H_2O(l)\rightarrow TiO_2(s)+4HCl(aq)[/tex]
3. [tex]NH_4NO_3(s)\rightarrow N_2(g)+O_2(g)+H_2O(g)[/tex]
The balanced equation is:
[tex]2NH_4NO_3(s)\rightarrow 2N_2(g)+O_2(g)+4H_2O(g)[/tex]
4.[tex] Ca3P2(s)+H2O(l)\rightarrow Ca(OH)2(aq)+PH3(g)[/tex]
The balanced equation is:
[tex] Ca_3P_2(s)+6H_2O(l)\rightarrow 3Ca(OH)_2(aq)+2PH_3(g)[/tex]
5. [tex]Al(OH)_3(s)+H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+H_2O(l)[/tex]
The balanced equation is:
[tex]2Al(OH)_3(s)+3H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+6H_2O(l)[/tex]
6.[tex] AgNO_3(aq)+Na_2SO_4(aq)\rightarrow Ag_2SO_4(s)+NaNO_3(aq)[/tex]
The balanced equation is:
[tex] 2AgNO_3(aq)+Na_2SO_4(aq)\rightarrow Ag_2SO_4(s)+2NaNO_3(aq)[/tex]
7. [tex]C_2H_5NH_2(g)+O_2(g)\rightarrow CO_2(g)+H_2O(g)+N_2(g)[/tex]
The balanced equation is:
[tex]4C_2H_5NH_2(g)+15O_2(g)\rightarrow 8CO_2(g)+14H_2O(g)+2N_2(g)[/tex]
A balanced chemical equation is a representation of a chemical reaction using chemical formulas and symbols, where the number of atoms of each element on the left side (reactants) is equal to the number of atoms of the same element on the right side (products). In other words, it obeys the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction
1. Li(s)+N2(g)→Li3N(s)
The balanced equation is :
[tex](Li(s) + N_2(g) \rightarrow Li_3N(s)\)[/tex]
2. TiCl4(l)+H2O(l)→TiO2(s)+HCl(aq)
The balanced equation is :
[tex]\(TiCl_4(l) + 4H_2O(l) \rightarrow TiO_2(s) + 4HCl(aq)\)[/tex]
3. NH4NO3(s)→N2(g)+O2(g)+H2O(g)
The balanced equation is :
[tex]\(NH_4NO_3(s) \rightarrow N_2(g) + 2O_2(g) + 2H_2O(g)\)[/tex]
4. Ca3P2(s)+H2O(l)→Ca(OH)2(aq)+PH3(g)
The balanced equation is :
[tex]\(Ca_3P_2(s) + 6H_2O(l) \rightarrow 3Ca(OH)_2(aq) + 2PH_3(g)\)[/tex]
5. Al(OH)3(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2O(l)
The balanced equation is :
[tex]\(2Al(OH)_3(s) + 3H_2SO_4(aq) \rightarrow Al_2(SO_4)_3(aq) + 6H_2O(l)\)[/tex]
6.AgNO3(aq)+Na2SO4(aq)→Ag2SO4(s)+NaNO3(aq)
The balanced equation is :
[tex]\(2AgNO_3(aq) + Na_2SO_4(aq) \rightarrow Ag_2SO_4(s) + 2NaNO_3(aq)\)[/tex]
7. C2H5NH2(g)+O2(g)→CO2(g)+H2O(g)+N2(g)
The balanced equation is :
[tex]\(2C_2H_5NH_2(g) + 9O_2(g) \rightarrow 4CO_2(g) + 10H_2O(g) + 2N_2(g)\)[/tex]
These equations show the balanced chemical reactions along with the respective phases of the substances involved.
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A single penny is 1.52 mm thick. The distance to the next nearest star other than our own (Alpha Centauri) is 4.22 light-years. If it were possible to stack one mole of pennies, how many times would the stack go between the earth and Alpha Centauri? Use the unit factoring method to determine the answer and show your work. You will need to find or look up the appropriate conversion factors to solve the problem. Your answer should be in scientific notation and have the correct number of significant figures in order to get full credit. (Please note that the text editing functions/buttons below for this essay question allows you to show exponents by using the button show as "x2"in the controls. To use it type the number followed by the exponent such as 104, highlight the 4 and hit the x2 button and you will end up with 104 as the result)
Answer:
2.29 × 10⁴ times
Explanation:
A single penny is 1.52 mm thick. The distance covered by 1 mole of pennies (6.02 × 10²³ pennies) is:
6.02 × 10²³ p × (1.52 mm/1 p) = 9.15 × 10²³ mm = 9.15 × 10²³ × 10⁻³ m = 9.15 × 10²⁰ m
The distance to the next nearest star other than our own (Alpha Centauri) is 4.22 light-years. Considering 1 ly = 9.46 × 10¹⁵ m, this distance in meters is:
4.22 ly × (9.46 × 10¹⁵ m/1 ly) = 3.99 × 10¹⁶ m
The times that the stack would go between the earth and Alpha Centauri are:
9.15 × 10²⁰ m / 3.99 × 10¹⁶ m = 2.29 × 10⁴
Determine the point groups for a. Naphthalene b. 1,8-Dichloronaphthalene c. 1,5-Dichloronaphthalene d. 1,2-Dichloronaphthalene
Answer:
a). Nepthalene is a D2h molecule because it has 3 C2 axes which are perpendicular and it has a mirror plane which is horizontal. Moreover C2 is taken as principal axis.
b). 1,8-dichloronaphthalene is a C2v molecule beccause it has 1 C2 axis, two rings are joined by the C-C bond and it also has two mirro planes.
c). 1,5-dichloronaphthalene is a C2h molecule because it has only 1 C2 axis which is pependicular to the plane, it has an inversion center and also a mirror plane which is horizontal in position.
d). 1,2-dichloronaphthalene is a Cs molecule because it has only a mirror plane.
Draw a structure containing only carbon and hydrogen that is a stable alkyne of five carbons containing a ring.
Answer:
Ethynylcyclopropane is the stable isomer for given alkyne.
Explanation:
In order to solve this problem we will first calculate the number of Hydrogen atoms. The general formula for alkynes is as,
CₙH₂ₙ₋₂
Putting value on n = 5,
C₅H₂.₅₋₂
C₅H₈
Also, the statement states that the compound contains one ring therefore, we will subtract 2 hydrogen atoms from the above formula i.e.
C₅H₈ ------------(-2 H) ----------> C₅H₆
Hence, the molecular formula for given compound is C₅H₆
Below, 4 different isomers with molecular formula C₅H₆ are attached.
The first compound i.e. ethynylcyclopropane is stable. As we know that alkynes are sp hybridized. The angle between C-C-H in alkynes is 180°. Hence, in this structure it can be seen that the alkyne part is linear and also the cyclopropane part is a well known moiety.
Compounds 3-ethylcycloprop-1-yne, cyclopentyne and 3-methylcyclobut-1-yne are highly unstable. The main reason for the instability is the presence of triple bond in three, five and four membered ring. As the alkynes are linear but the C-C-H bond in these compound is less than 180° which will make them highly unstable.
What mass of Na2CrO4 is required to precipitate all of the silver ions from 73.6 mL of a 0.150 M solution of AgNO3?
Answer:
We need 0.894 grams of Na2CrO4
Explanation:
Step 1: Data given
Volume of a 0.150 M AgNO3 = 73.6 mL = 0.0736 L
Step 2: Calculate moles of Ag+
Moles Ag+ = moles AgNO3
Moles Ag+ = volume * molarity
moles Ag+ = 0.0736 L x 0.150 M = 0.01104 moles
Step 3: Calculate moles Na2CrO4
2AgNO3 + Na2CrO4 → Ag2CrO4 (s) + 2NaNO3
For 2 moles AgNO3 we need 1 mol Na2CRO4
For 0.01104 moles AgNO3 we need 0.01104/2 = 0.00552 moles Na2CrO4
Step 4: Calculate mass of Na2CrO4
Mass Na2CrO4 = moles * molar mass
Mass Na2CrO4 = 0.00552 moles * 161.97 g/mol
Mass Na2CrO4 = 0.894 grams
We need 0.894 grams of Na2CrO4
To precipitate all the silver ions, 0.893 g of Na2CrO4 is required.
Explanation:To calculate the mass of Na2CrO4 required to precipitate all of the silver ions from the solution, we need to use the stoichiometry of the reaction. The balanced equation for the reaction is:
2AgNO3 + Na2CrO4 → Ag2CrO4 + 2NaNO3
From the equation, we can see that 2 moles of AgNO3 react with 1 mole of Na2CrO4 to form 1 mole of Ag2CrO4. The molarity of AgNO3 is given as 0.150 M and the volume is 73.6 mL. First, we need to convert the volume to liters:
73.6 mL × (1 L / 1000 mL) = 0.0736 L
Next, we can use the molarity and volume to calculate the number of moles of AgNO3:
moles of AgNO3 = molarity × volume = 0.150 M × 0.0736 L = 0.01104 moles
Since the reaction ratio is 2 moles of AgNO3 to 1 mole of Na2CrO4, we can calculate the number of moles of Na2CrO4:
moles of Na2CrO4 = (0.01104 moles of AgNO3) / 2 = 0.00552 moles
Finally, we can use the molar mass of Na2CrO4 to calculate the mass:
mass of Na2CrO4 = moles of Na2CrO4 × molar mass of Na2CrO4
From the periodic table, the molar mass of Na2CrO4 is:
molar mass of Na2CrO4 = 22.99 g/mol + (2 × 35.45 g/mol) + 4 × 16.00 g/mol = 161.97 g/mol
Therefore, the mass of Na2CrO4 required to precipitate all of the silver ions is:
mass of Na2CrO4 = 0.00552 moles × 161.97 g/mol = 0.893 g
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Citrus fruits are rich in citric acid, a compound with three COOH groups. Explain the following: a. The first pKa (for the COOH group in the center of the molecule) is lower than the pKa of acetic acid. b. The third pKa is greater than the pKa of acetic acid.
Answer:
a. the first pKa is lower because of the presence of an electron withdrawing 'OH' group attached to the carbon that is directly attached to it.
b. the third pKa is greater than that of acetic acid because of the presence of an electron donating methyl group which is directly attached to it.
Explanation:
Induction or Inductive effect is the electronic effects an atom or a group of atoms exert on a compound or a portion of a compound, which could either be electron donating or electron withdrawing, thereby affecting its acidity or basicity.
Electronegativity confers acidity on a compound. In a, the OH group withdraws electrons from the COOH group, conferring more electronegativity on the middle COOH group, thereby reducing the pKa and thus increasing acidity.
In b, the electron donating effect of the methyl group, decreases the electronegativity of the COOH group,p thereby increasing the pKa which also means decreased acidity.
The first pKa of citric acid is lower than acetic acid due to the presence of three COOH groups. The third pKa of citric acid is greater than acetic acid due to steric hindrance caused by the presence of two COOH groups at either end of the molecule.
Explanation:a. The first pKa of citric acid is lower than the pKa of acetic acid due to the presence of three COOH groups. The proximity of the COOH groups in citric acid allows for easier liberation of the H+ ions, resulting in a lower pKa value. This is supported by the concept of resonance stabilization. In contrast, acetic acid has only one COOH group, resulting in a higher pKa value.
b. The third pKa of citric acid is greater than the pKa of acetic acid due to steric hindrance caused by the presence of two COOH groups at either end of the molecule. The close proximity of these two groups makes it difficult for the liberation of the H+ ion, resulting in a higher pKa value compared to acetic acid.
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Consider the second-order reaction: 2HI(g)→H2(g)+I2(g). Use the simulation to find the initial concentration [HI]0and the rate constant k for the reaction. What will be the concentration of HI after t = 1.01×10^10 s ([HI]t) for a reaction starting under the condition in the simulation?
Explanation:
The given reaction equation is as follows.
[tex]2HI(g) \rightarrow H_{2}(g) + I_{2}(g)[/tex]
[tex]\frac{-d[HI]}{dt} = k[HI]^{2}[/tex]
[tex]-\int_{[HI]_{o}}^{[HI]_{t}} \frac{d[HI]}{[HI]^{2}} = k \int_{o}^{t} dt[/tex]
[tex]-[\frac{-1}{[HI]}]^{[HI]_{t}}_{[HI]_{o}} = kt[/tex]
[tex]\frac{1}{[HI]_{t}} - \frac{1}{[HI]_{o}} = kt[/tex] .......... (1)
where, [tex][HI_{o}][/tex] = Initial concentration
[tex][HI]_{t}[/tex] = concentration at time t
k = rate constant
t = time
Now, we will calculate the initial concentration of HI as follows.
Initial rate = [tex]1.6 \times 10^{-7} mol/sec[/tex]
k = [tex]6.4 \times 10^{-9}[/tex]
R = [tex]k[HI]^{2}_{o}[/tex]
[tex][HI]^{2}_{o} = \frac{R}{k}[/tex]
= [tex]\frac{1.6 \times 10^{-7}}{6.4 \times 10^{-9}}[/tex]
[tex][HI]_{o}[/tex] = 5 M
Now, we will calculate the concentration of [tex][HI]_{t}[/tex] at t = [tex]1.01 \times 10^{10}[/tex] sec as follows.
Using equation (1) as follows.
k = [tex]6.4 \times 10^{-9}[/tex]
[tex]\frac{1}{[HI]_{t}} - \frac{1}{5}[/tex] = [tex](6.4 \times 10^{-9}) \times 1.01 \times 10^{10}[/tex]
[tex]\frac{1}{[HI]_{t}}[/tex] = 64.44
[tex][HI]_{t}[/tex] = 0.0155 M
Thus, we can conclude that concentration of HI at t = [tex]1.01 \times 10^{10}[/tex] sec is 0.0155 M.
A reception subservient on the second and first-order reactants is called a second-order reaction.
The correct answer is:
The concentration of HI at t = 1.01 × 10¹⁰ sec is 0.0155 M.
The equation according to the question is:
2 HI (g) ⇒ H₂ (g) + I₂ (g)
[tex]\dfrac{\text{-d}\left[\begin{array}{ccc}\text{HI}\end{array}\right] }{\text{dt}} & = \text{k} \left[\begin{array}{ccc}\text{HI}\end{array}\right] ^{2}[/tex]
[tex]\dfrac{1}{\left[\begin{array}{ccc}\text{HI}\end{array}\right] _{\text{t}} } - \dfrac{1}{\left[\begin{array}{ccc}\text{HI}\end{array}\right] _{\text{o}} } &= \text{kt}[/tex] .......equation (1)
Where, the initial concentration can be represented as: [tex]\left[\begin{array}{ccc}\text{HI}_{o} \end{array}\right][/tex]
The concentration at time t = [tex]\left[\begin{array}{ccc}\text{HI}\end{array}\right] \text{t}[/tex]
Rate constant will be = k
The time will be = t
The initial concentration of HI can be calculated as:
The initial rate = 1.6 × 10⁻⁷ mol/sec
k = 6.4 × 10⁻⁹
[tex]\text{R} & = \text{k} \left[\begin{array}{ccc}\text{HI}\end{array}\right] ^{2} _{0}[/tex]
[tex]\dfrac{\text{R}}{\text{k}} & =\left[\begin{array}{ccc}\text{HI}\end{array}\right] ^{2} _{0}[/tex]
= [tex]\dfrac{1.6 \times 10^{-7} }{6.4 \times 10^{-9} }[/tex]
[tex]\left[\begin{array}{ccc}\text{HI}\end{array}\right]\end{array}\right] _{0} &= 5 \;\text{M}[/tex]
To calculate the concentration [tex]\left[\begin{array}{ccc}\text{HI}\end{array}\right] \text{t}[/tex] at time (t) = 1.01 × 10 ¹⁰ sec.
Now, using the above equation: (1)
k = 6.4 × 10⁻⁹
[tex]\dfrac{1}{\left[\begin{array}{ccc}\text{HI}\end{array}\right] \text{t}} - \dfrac{1}{5}[/tex]
= (6.4 × 10⁻⁹) × 1.01 × 10¹⁰
[tex]\dfrac{1}{\left[\begin{array}{ccc}\text{HI}\end{array}\right] \text{t}} = 64.44[/tex]
[tex]{\left[\begin{array}{ccc}\text{HI}\end{array}\right] \text{t}} = 0.0155 \;\text{M}[/tex]
Therefore, concentration of HI at t = 1.01 × 10¹⁰ sec is 0.0155 M.
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Increasing the amount of water in which the sugar is dissolved will increase the frequency of collisions between the sucrose molecules and the water molecules resulting in an increase in the rate of hydrolysis.
True or false?
Answer: The given statement is true.
Explanation:
When we increase the amount of solvent which is water in this case then it means there will occur an increase in the molecules. Hence, there will be more number of collisions to take place with increase in number of molecules.
Therefore, more is the amount of interaction taking place between the molecules of a solution more will be its rate of hydrolysis.
Thus, we can conclude that the statement increasing the amount of water in which the sugar is dissolved will increase the frequency of collisions between the sucrose molecules and the water molecules resulting in an increase in the rate of hydrolysis, is true.
The half-life of a radioactive isotope is the amount of time it takes for a quantity of radioactive material to decay to one-half of its original amount.
Answer: The statement is true
Explanation:
The half-life of a radioactive isotope is the time taken for half of the total number of atoms in a given sample of the isotope to decay.
For instance
The half-life of radium is 1622 years. This means that if we have 1000 radium atoms at the beginning, then at the end of 1622 years, 500 atoms would have disintegrated, leaving 500 undecayed radium atoms
Thus, the statement is true
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46Ti 70.600% 45.95263 48Ti 11.900% 47.94795 50Ti 17.500% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass = 47.867
Final answer:
The average atomic mass of titanium on the hypothetical planet is calculated by using the weighted average of the abundances and masses of its isotopes, resulting in 46.8989 amu.
Explanation:
The average atomic mass of titanium on that hypothetical planet can be calculated by multiplying the abundance of each isotope by its mass (in atomic mass units, amu), then summing these products. The calculation will look as follows:
(0.70600 × 45.95263 amu) for 46Ti(0.11900 × 47.94795 amu) for 48Ti(0.17500 × 49.94479 amu) for 50TiTo find the average atomic mass, we add these values together to get the sum which should give us the average atomic mass of titanium on the planet.
The correct calculation would be:
(0.70600 × 45.95263 amu) + (0.11900 × 47.94795 amu) + (0.17500 × 49.94479 amu)= (32.45785 amu) + (5.70081 amu) + (8.74024 amu)= 46.8989 amuHence, the average atomic mass of titanium for this planet is 46.8989 amu. It's important to note that the average atomic mass of an element is the weighted average of all the isotopes of that element.
g The decomposition reaction of A to B is a first-order reaction with a half-life of 2.42×103 seconds: A → 2B If the initial concentration of A is 0.163 M, how many minutes will it take for the concentration of A to be 66.8% of the initial concentration?
Answer:
In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.
Explanation:
The equation used to calculate the constant for first order kinetics:
[tex]t_{1/2}=\frac{0.693}{k}}[/tex] .....(1)
Rate law expression for first order kinetics is given by the equation:
[tex]t=\frac{2.303}{k}\log\frac{[A_o]}{[A]}[/tex] ......(2)
where,
k = rate constant
[tex]t_{1/2}[/tex] =Half life of the reaction = [tex]2.42\times 10^3 s[/tex]
t = time taken for decay process = ?
[tex][A_o][/tex] = initial amount of the reactant = 0.163 M
[A] = amount left after time t = 66.8% of [tex][A_o][/tex]
[A]=[tex]\frac{66.8}{100}\times 0.163 M=0.108884 M[/tex]
[tex]k=\frac{0.693}{2.42\times 10^3 s}[/tex]
[tex]t=\frac{2.303}{\frac{0.693}{2.42\times 10^3 s}}\log\frac{0.163 M}{0.108884 M}[/tex]
t = 1,409.19 s
1 minute = 60 sec
[tex]t=\frac{1,409.19 }{60} min=23.49 min[/tex]
In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.
Write the rate law for the reaction 2A + B → C if the reaction
(1) is second order in B and overall third order, –rA = ______
(2) is zero order in A and first order in B, –rA = ______
(3) is zero order in both A and B, –rA = ______
(4) is first order in A and overall zero order. –rA = ______
Answer:
1. [tex]R=k[A]^1[B]^2[/tex]
2. [tex]R=k[B]^1[/tex]
3. [tex]R=k[A]^0[B]^0=k[/tex]
4. [tex]R=k[A]^1[B]^{-1}[/tex]
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
(1) is second order in B and overall third order.
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= x + 2 = 3
x = 1
Rate of the reaction =R
[tex]R=k[A]^1[B]^2[/tex]
(2) is zero order in A and first order in B.
2A + B → C
Rate of the reaction =R
[tex]R=k[A]^0[B]^1=k[B]^1[/tex]
Order of the reaction = sum of stoichiometric coefficient
= 0 + 1 = 1
(3) is zero order in both A and B .
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= 0 + 0 = 0
Rate of the reaction =R
[tex]R=k[A]^0[B]^0=k[/tex]
(4) is first order in A and overall zero order.
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= 1 + x = 0
x = -1
Rate of the reaction = R
[tex]R=k[A]^1[B]^{-1}[/tex]
What is the molarity of a 10.5 %% by mass glucose (C6H12O6C6H12O6) solution? (The density of the solution is 1.03 g/mLg/mL .) Express your answer to three significant figures.
The molarity of the 10.5% by mass glucose solution is 0.600 M.
Explanation:To find the molarity of the glucose solution, we need to determine the number of moles of glucose present in the solution first. We can use the percent by mass to calculate this.
Given that the solution is 10.5% by mass, we know that 10.5 grams of glucose is present in a 100 gram solution. We can convert this to moles by dividing the mass of glucose by its molar mass, which is 180.16 g/mol.
So, the number of moles of glucose is 10.5 g / 180.16 g/mol = 0.0583 mol. To find the molarity, we divide the number of moles by the volume of the solution in liters. The volume of the solution can be determined by multiplying the density of the solution by its mass: 100 g / (1.03 g/mL) = 97.09 mL = 0.0971 L.
Therefore, the molarity of the glucose solution is 0.0583 mol / 0.0971 L = 0.600 M.
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The molarity of a 10.5% by mass glucose solution with a density of 1.03 g/mL can be calculated by assuming a 100 g sample of the solution. The mass of glucose per liter is found to be 108.1395 g, and with the molar mass of glucose, the molarity is determined to be 0.600 M.
The question pertains to determining the molarity of a 10.5% by mass glucose solution with a given density of 1.03 g/mL. To calculate the molarity, we need to use the given mass percentage and density to find out how many moles of glucose are present in a liter of solution.
First, assume you have 100 g of this solution. Because it's a 10.5% by mass solution, this means there are 10.5 g of glucose (C6H12O6) and 89.5 g of water in the mixture.
Using the density, we find the volume of 100 g of solution:
100g / 1.03g/mL = 97.09 mL
Because we want to know the molarity per liter, it's important to work with a liter of the solution:
(1000 mL/L) / (97.09 mL) = 10.299 L^-1 multiplication factor
Now, we will use the multiplication factor to scale up the mass of glucose to what would be in one liter:
10.5 g * 10.299 = 108.1395 g glucose per liter
The molar mass of glucose (C6H12O6) is approximately 180.16 g/mol, so the number of moles in one liter would be:
108.1395 g / 180.16 g/mol = 0.600 mol/L
Therefore, the molarity of the glucose solution is 0.600 M.
A 20.3 mass % aqueous solution of iron(III) chloride has a density of 1.280 g/mL. Calculate the molality of the solution. Give your answer to 2 decimal places.
Answer:
Molality for the solution is 1.57 m
Explanation:
Molality is mol of solute in 1kg of solvent.
20.3 % by mass means that 20.3 g of solute (FeCl₃) are contained in 100 g of solution..
Let's determine the mass of solvent.
Mass of solution = Mass of solvent + Mass of solute
100 g = Mass of solvent + 20.3 g
100 g - 20.3 g = Mass of solvent → 79.7 g
Let's convert the mass in g to kg
79.7 g . 1kg / 1000 g = 0.0797 kg
Let's determine the moles of solute (mass / molar mass)
20.3 g / 162.2 g/mol = 0.125 mol
Molality = 0.125 mol / 0.0797 kg → 1.57 m
Final answer:
The molality of the 20.3% aqueous solution of iron(III) chloride is 1.60 m.
Explanation:
This question demands basic understanding of molatility.
To calculate the molality of the solution, we need to determine the moles of solute (iron(III) chloride) and the mass of the solvent (water).
First, convert the mass percent to grams of solute:
Mass of solute = (20.3%)(1.280 g/mL)(1000 mL) = 260.48 g
Next, calculate the moles of solute:
Moles of solute = (260.48 g)/(162.2 g/mol) = 1.603 mol
Finally, calculate the molality:
Molality = (1.603 mol)/(1 kg) = 1.60 m
Therefore, The molality of the 20.3% aqueous solution of iron(III) chloride is 1.60 m.
Naturally occurring iodine has an atomic mass of 126.9045 amu. A 12.3849-g sample of iodine is accidentally contaminated with 1.00070 g of 129I, a synthetic radioisotope of iodine used in the treatment of certain diseases of the thyroid gland. The mass of 129I is 128.9050 amu. Find the apparent "atomic mass" of the contaminated iodine.
The apparent "atomic mass" of the contaminated iodine is approximately 1111.9285 amu.
To determine the apparent "atomic mass" of contaminant iodine, we need to take into account the contribution of both the naturally occurring iodine ([tex]\rm ^1^2^7I[/tex]) and the man-made radioisotope ([tex]\rm ^1^2^9I[/tex]).
The formula for calculating the atomic mass is:
Atomic mass = (mass of isotope 1 * abundance of isotope 1) + (mass of isotope 2 * abundance of isotope 2) + ...
Lets calculating the abundances of [tex]\rm ^1^2^7I[/tex] and [tex]\rm ^1^2^9I[/tex]:
Abundance of [tex]\rm ^1^2^7I[/tex] = 1 - Abundance of [tex]\rm ^1^2^9I[/tex]
Given:
Mass of [tex]\rm ^1^2^7I[/tex] = 126.9045 amu
Mass of [tex]\rm ^1^2^9I[/tex] = 128.9050 amu
We have two isotopes: [tex]\rm ^1^2^7I[/tex] and [tex]\rm ^1^2^9I[/tex]. The masses of these isotopes and their abundances need to be considered:
Atomic mass = (mass of [tex]\rm ^1^2^7I[/tex] * abundance of [tex]\rm ^1^2^7I[/tex]) + (mass of [tex]\rm ^1^2^9I[/tex]* abundance of [tex]\rm ^1^2^9I[/tex])
We need to calculate the abundances of [tex]\rm ^1^2^7I[/tex] and [tex]\rm ^1^2^9I[/tex] before we can calculate the atomic mass.
Mass of contaminated iodine sample = 12.3849 g + 1.00070 g = 13.3856 g
Now we can calculate the abundances:
Abundance of [tex]\rm ^1^2^7I[/tex] = (mass of [tex]I-127[/tex] in sample) / (total mass of sample)
Abundance of [tex]\rm ^1^2^7I[/tex] = (12.3849 g * 126.9045 amu) / (13.3856 g) = 117.0997 amu / 13.3856 g ≈ 8.7411
Abundance of [tex]\rm ^1^2^9I[/tex] = (mass of I-129 in sample) / (total mass of sample)
Abundance of [tex]\rm ^1^2^9I[/tex]= (1.00070 g * 128.9050 amu) / (13.3856 g) = 128.9050 amu / 13.3856 g ≈ 9.6175
We can calculate the atomic mass:
Atomic mass = (126.9045 amu * 8.7411) + (128.9050 amu * 9.6175) ≈ 1111.9285
Therefore, the apparent "atomic mass" of the contaminated iodine is approximately 1111.9285 amu.
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The apparent atomic mass of the contaminated iodine is 126.9045 amu.
Explanation:
To calculate the apparent atomic mass of the contaminated iodine, we can use the formula:
Apparent atomic mass = (mass of naturally occurring iodine * atomic mass of naturally occurring iodine + mass of synthetic radioisotope * atomic mass of synthetic radioisotope) / total mass of contaminated iodine
Given:
Mass of naturally occurring iodine = 12.3849 gAtomic mass of naturally occurring iodine = 126.9045 amuMass of synthetic radioisotope = 1.00070 gAtomic mass of synthetic radioisotope = 128.9050 amuSubstituting the given values into the formula:
Apparent atomic mass = (12.3849 g * 126.9045 amu + 1.00070 g * 128.9050 amu) / (12.3849 g + 1.00070 g)
Simplifying the expression:
Apparent atomic mass = (1570.6078055 + 128.905070) / 13.3856
Apparent atomic mass = 1699.5128755 / 13.3856
Apparent atomic mass = 126.9045 amu
Therefore, the apparent atomic mass of the contaminated iodine is 126.9045 amu.
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A liquid is added to a buret, and the initial measurement is found to be 0.75 mL. After liquid has been added to the flask from the buret, the buret reads 15.20 mL. How much liquid (in mL) was dispensed from the buret, with the correct number of significant figures?
Answer:
14.45 mL
Explanation:
The rule apply for the addition and subtraction for significant digits is :
The least precise number present after the decimal point determines the number of significant figures in the answer.
Initial Burette reading = 0.75 mL ( 2 significant digits)
Final Burette reading = 15.20 mL ( 4 significant digits)
Liquid dispensed = 15.20 mL - 0.75 mL = 14.45 mL ( Answer to two decimal places )
To find the amount of liquid dispensed from the buret, subtract the initial volume (0.75 mL) from the final volume (15.20 mL), resulting in 14.45 mL of liquid dispensed. Ensure that the answer is reported with the same level of precision as the measurements from the buret.
Explanation:To calculate the amount of liquid dispensed from the buret, you subtract the initial measurement from the final measurement. In this case, the initial measurement is 0.75 mL and the final measurement after the liquid is added to the flask is 15.20 mL. Therefore, the amount of liquid dispensed is 15.20 mL - 0.75 mL = 14.45 mL.
Burets are commonly used in titration analyses and allow volume measurements to the nearest 0.01 mL, which is why our final answer should be reported with the same level of precision as the buret readings. According to the proper significant figures rules, the result should be reported with the same number of decimal places as the measurement with the fewest decimal places. Since the readings from the buret are given to two decimal places (0.75 mL and 15.20 mL), our calculated volume of dispensed liquid also should be reported to two decimal places as 14.45 mL.
What feature of an orbital is related to each of the following quantum numbers?
(a) Principal quantum number (n)
(b) Angular momentum quantum number (l)
(c) Magnetic quantum number (ml)
Each of the following quantum numbers is related to an orbital characteristic in the following ways: n, the primary quantum number
What is quantum number?The values of conserved quantities in the dynamics of a quantum system are explained by quantum numbers in quantum physics and chemistry.Quantum numbers can be used to describe the electrons in atomic orbitals. An atom's or ion's electron has four quantum numbers that characterize its state. Consider the electrons as important variables in an equation that describes the three-dimensional position of the electrons in a certain atom. The primary quantum number (n), the orbital angular momentum quantum number (l), the magnetic quantum number (ml), and the electron spin quantum number are the four quantum numbers that make up an atom (ms).To learn more about quantum number refer to:
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Final answer:
The principal quantum number determines the energy range and distance of an electron from the nucleus. The angular momentum quantum number determines the shape or type of the orbital. The magnetic quantum number determines the orientation of the orbital in space.
Explanation:
The feature of an orbital related to the principal quantum number (n) is the general range for the value of energy and the probable distances that the electron can be from the nucleus.
The feature of an orbital related to the angular momentum quantum number (l) is the shape or type of the orbital. The values of 1 range from 0 to (n-1), and orbitals with the same principal quantum number and the same l value belong to the same subshell.
The feature of an orbital related to the magnetic quantum number (m₁) is the orientation of the orbital in space. The values of m₁ range from -l to +l, and orbitals with the same l value have different orientations.
Draw the partial (valence-level) orbital diagram, and write the symbol, group number, and period number of the element:
(a) [Ne] 3s²3p⁵
(b) [Ar] 4s²3d¹⁰4p³
Answer:
a) Element = Chlorine
b) Element = Arsenic
Explanation:
The knowledge of Orbitals and Quantum number and the electronic configuration is applied as shown in the analysis in the attached file.
A student ran the following reaction in the laboratory at 600 K: COCl2(g) CO(g) + Cl2(g) When he introduced COCl2(g) at a pressure of 0.822 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of COCl2(g) to be 0.351 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.
The equilibrium constant, Kp, for the reaction COCl2(g) → CO(g) + Cl2(g) at 600 K is calculated to be 0.634.
Explanation:To calculate the equilibrium constant, Kp, for the reaction COCl2(g) → CO(g) + Cl2(g) at 600 K, we must first use the given equilibrium partial pressure of COCl2(g) to determine the change in pressure for CO and Cl2 since the reaction started with only COCl2 present. The initial pressure of COCl2 was 0.822 atm, and the equilibrium partial pressure was 0.351 atm, which implies the pressure change (∆P) for CO and Cl2 is 0.822 atm - 0.351 atm = 0.471 atm.
Since the reaction shows that 1 mole of COCl2 produces 1 mole of CO and Cl2 each, the equilibrium partial pressures of CO and Cl2 are also 0.471 atm each. Now, we can write the expression for Kp, which is Kp = (PCO)(PCl2) / (PCOCl2). Plugging in the values, we get Kp = (0.471 atm)(0.471 atm) / (0.351 atm), and thus Kp is calculated to be 0.634 at 600 K.
A 1.00-kg block of copper at 100°C is placed in an in- sulated calorimeter of negligible heat capacity containing 4.00 L of liquid water at 0.0°C. Find the entropy change of (a) the cop- per block, (b) the water, and (c) the universe.
Answer:
the entropy change of the copper block = - 117.29 J/K
the entropy change of the water = 138.01 J/K
the entropy change of the universe = 20.72 J/K
Explanation:
For Copper block:
the mass of copper block [tex](m_c)[/tex] = 1.00 kg
Temperature of block of copper [tex](T_c)[/tex] = 100°C
= (100+273)K
= 373K
Standard Heat capacity for copper [tex](C_c)[/tex] = 386 J/kg.K
For water:
We know our volume of liquid water to be = 4.00 L
At 0.0°C Density of liquid water = 999.9 kg/m³
As such; we can determine the mass since : [tex]density = \frac{mass}{volume}[/tex]
∴ the mass of 4.00 L of liquid water at 0.0°C will be its density × volume.
= 999.9 kg/m³ × [tex]\frac{4}{1000}m^3[/tex]
= 3.9996 kg
so, mass of liquid water [tex](m_w)[/tex] = 3.9996 kg
Temperature of liquid water [tex](T_w)[/tex] at 0.0°C = 273 K
Standard Heat Capacity of liquid water [tex](C_w)[/tex] = 4185.5 J/kg.K
Let's determine the equilibruium temperature between the copper and the liquid water. In order to do that; we have:
[tex]m_cC_c \delta T_c =m_wC_w \delta T_w[/tex]
[tex]1.00*386*(373-T_\theta)=3.996*4185.5*(T _\theta-273)[/tex]
[tex]386(373-T_\theta)=16725.26(T_\theta-273)[/tex]
[tex](373-T_\theta)=\frac{16725.26}{386} (T_\theta-273)[/tex]
[tex](373-T_\theta)=43.33 (T_\theta-273)[/tex]
[tex](373-T_\theta)=43.33 T_\theta-11829.09[/tex]
[tex]373+11829.09=43.33 T_\theta+T_\theta[/tex]
[tex]12202.09 =43.33T_\theta[/tex]
[tex]T_\theta= 275.26 K[/tex]
∴ the equilibrium temperature = 275.26 K
NOW, to determine the Entropy change of the copper block; we have:
[tex](\delta S)_{copper}=m_cC_cIn(\frac{T_\theta}{T_c} )[/tex]
[tex](\delta S)_{copper}=1.0*386In(\frac{275.26}{373} )[/tex]
[tex](\delta S)_{copper}=-117.29 J/K[/tex]
The entropy change of the water can also be calculated as:
[tex](\delta S)_{water}=m_wC_wIn(\frac{T_\theta}{T_w} )[/tex]
[tex](\delta S)_{water}=3.9996*4185.5In(\frac{275.26}{373} )[/tex]
[tex](\delta S)_{water}=138.01J/K[/tex]
The entropy change of the universe is the combination of both the entropy change of copper and water.
[tex](\delta S)_{universe}=(\delta S)_{copper}+(\delta S)_{water}[/tex]
[tex](\delta S)_{universe}=(-117.29+138.01)J/K[/tex]
[tex](\delta S)_{universe}=20.72J/K[/tex]
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq)HCl(aq), as described by the chemical equationMnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g)MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g)How much MnO2(s)MnO2(s) should be added to excess HCl(aq)HCl(aq) to obtain 115 mL Cl2(g)115 mL Cl2(g) at 25 °C and 805 Torr805 Torr?
Answer:
4.98 × 10⁻³ mol
Explanation:
Given data for Cl₂
Volume (V): 115 mL = 0.115 LPressure (P): 1.06 atm[tex]805torr.\frac{1atm}{760torr} =1.06atm[/tex]
Temperature (T): 25°C + 273.15 = 298 KFirst, we will calculate the moles of Cl₂ using the ideal gas equation.
P × V = n × R × T
n = P × V / R × T
n = 1.06 atm × 0.115 L / (0.0821 atm.L/mol.K) × 298 K
n = 4.98 × 10⁻³ mol
Let's consider the balanced equation.
MnO₂(s) + 4 HCl(aq) ⟶ MnCl₂(aq) + 2 H₂O(l) + Cl₂(g)
The molar ratio of MnO₂ to Cl₂ is 1:1. The required moles of MnO₂ are 4.98 × 10⁻³ moles.
The volume of 1 kg of helium in a piston-cylinder device is initially 5 m3 . Now helium is compressed to 2 m3 while its pressure is maintained constant at 180 kPa. Determine the work required to compress helium, in kJ.
Answer: The work required to compress helium gas is 540 kJ
Explanation:
To calculate the amount of work done for an isothermal process is given by the equation:
[tex]W=-P\Delta V=-P(V_2-V_1)[/tex]
W = amount of work done = ?
P = pressure = 180 kPa
[tex]V_1[/tex] = initial volume = [tex]5m^3[/tex]
[tex]V_2[/tex] = final volume = [tex]2m^3[/tex]
Putting values in above equation, we get:
[tex]W=-180kPa\times (2-5)m^3=540kPa.m^3[/tex]
To convert this into joules, we use the conversion factor:
[tex]1kPa.m^3=1kJ[/tex]
So, [tex]540kPa.m^3=540kJ[/tex]
The positive sign indicates that work is done by the system.
Hence, the work required to compress helium gas is 540 kJ
The work required to compress 1 kg of helium from 5 m³ to 2 m³ at a constant pressure of 180 [tex]K_p_a[/tex] is 540 kJ.
This problem involves the calculation of work done during the compression of helium gas in a piston-cylinder device at a constant pressure. The work required to compress the gas can be determined using the formula for work done by a gas at constant pressure:
Work (W) = P x ΔV
Where:
P is the pressure, which is 180 [tex]K_p_a[/tex] (or 180 kJ/m³).ΔV (change in volume) is the difference in volume, which is the initial volume minus the final volume.Thus, ΔV = [tex]V_i_n_i_t_i_a_l[/tex] - [tex]V_f_i_n_a_l[/tex]
Given:
Initial volume, [tex]V_i_n_i_t_i_a_l[/tex] = 5 m³Final volume, [tex]V_f_i_n_a_l[/tex] = 2 m³Therefore:
ΔV = 5 m³ - 2 m³ = 3 m³
Substituting the values into the work formula:
Work (W) = 180 [tex]K_p_a[/tex] x 3 m³ = 540 kJ
Therefore, the work required to compress the helium is 540 kJ.
Potassium (K) has a work function value of 2.29 eV. What is the wavelength of light required to begin to generate a current in an apparatus like the one Hertz used with potassium metal?
Answer: The wavelength of light required is [tex]5.43\times 10^{-7}m[/tex]
Explanation:
To calculate the threshold wavelength for a given work function, we use the equation:
[tex]\phi =h\nu_o[/tex]
where,
[tex]\phi[/tex] = work function of the potassium metal = [tex]2.29eV=3.66\times 10^{-19}J[/tex] (Conversion factor: [tex]1eV=1.6\times 10^{-19}[/tex] )
h = Planck's constant = [tex]6.626\times 10^{-34}Js[/tex]
[tex]\nu_o=\frac{c}{\lambda _o}[/tex]
c = speed of light = [tex]3\times 10^9m/s[/tex]
[tex]\lambda_o[/tex] = wavelength of light
Putting values in above equation:
[tex]3.66\times 10^{-19}J=\frac{6.626\times 10^{-34}Js\times 3\times 10^8m/s}{\lambda_o}\\\\\lambda_o=\frac{6.626\times 10^{-34}Js\times 3\times 10^8m/s}{3.66\times 10^{-19}J}=5.43\times 10^{-7}m[/tex]
Hence, the wavelength of light required is [tex]5.43\times 10^{-7}m[/tex]
A sample of uranium ore contains 6.73 mg of 238U and 3.22 mg of 206Pb. Assuming all of the lead arose from the decay of the uranium and that the half-life of 238U is 4.51 x 109years, determine the age of the ore
Answer:
The age of the ore is 4.796*10^9 years.
Explanation:
To solve this question, we use the formula;
A(t) =A(o)(1/2)^t/t1/2
where;
A(t) =3.22mg
A(o) = 6.731mg
t1/2 = 4.51*70^9 years
t = age of the ore
So,
A(t) =A(o)(1/2)^t/t1/2
3.22 = 6.73 (1/2)^t/4.51*10^9
Divide both sides by 6.73
3.22/6.73= (1/2)^t/4.51*10^9
0.47825= (0.5)^t/4.51*10^9
Log 0.4785 = t/4.51*10^9 • log 0.5
Log 0.4785/log 0.5 • 4.51*10^9 = t
t = 1.0634 * 4.51*10^9
t = 4.796*10^9
So therefore, the age of the ore is approximately 4.796*10^9 years.