Calculate the mass of 1.9 • 10^24 atoms of Pb

Answer:

The answer to your question is   C₃H₆O

Explanation:

Data

mass of sample = 23.2 g

mass of carbon dioxide = 52.8 g

mass of water = 21.6 g

empirical formula = ?

Process

1.- Calculate the mass and moles of carbon

                       44 g of CO₂ ---------------  12 g of C

                        52.8 g          ---------------  x

                        x = (52.8 x 12)/44

                        x = 633.6/44

                        x = 14.4 g of C

                        12 g of C ------------------  1 mol

                        14.4 g of C ---------------   x

                         x = (14.4 x 1)/(12)

                         x = 1.2 moles of C

2.- Calculate the grams and moles of Hydrogen

                         18 g of H₂O ---------------  2 g of H

                         21.6 g of H₂O -------------  x

                          x = (21.6 x 2) / 18

                         x = 2.4 g of H

                         1 g of H -------------------- 1 mol of H

                         2.4 g of H -----------------  x

                          x = (2.4 x 1)/1

                          x = 2.4 moles of H

3.- Calculate the grams and moles of Oxygen

Mass of Oxygen = 23.2 - 14.4 - 2.4

                           = 6.4 g

                         16 g of O ----------------  1 mol

                          6.4 g of O --------------  x

                          x = (6.4 x 1)/16

                          x = 0.4 moles of Oxygen

4.- Divide by the lowest number of moles

Carbon = 1.2 / 0.4 = 3

Hydrogen = 2.4/ 0.4 = 6

Oxygen = 0.4 / 0.4 = 1

5.- Write the empirical formula

                                C₃H₆O

Final answer:

To find the empirical formula of a compound from its combustion products, convert the masses of carbon dioxide and water to moles to determine the moles of carbon, hydrogen, and oxygen in the compound. Calculating these mole ratios leads to determining that the empirical formula of the compound is C3H6O.

Explanation:

To determine the empirical formula of the compound given its combustion products, begin by converting the mass of carbon dioxide (CO2) and water (H2O) to moles. This reveals the moles of carbon and hydrogen in the original compound. Since oxygen is also part of the compound, calculate its moles by subtraction from the total mass of the original compound.

Convert 52.8 g of CO2 to moles: (52.8 g) / (44.01 g/mol) = 1.2 mol of C.Convert 21.6 g of H2O to moles: (21.6 g) / (18.015 g/mol) = 1.2 mol of H2, or 2.4 mol of H.Calculate moles of oxygen in the compound: Subtract the mass of C and H in the original compound from its total mass. Mass of C from CO2 = 1.2 mol × 12 g/mol = 14.4 g; Mass of H from H2O = 2.4 mol × 1 g/mol = 2.4 g. Total mass of C and H = 14.4 g + 2.4 g = 16.8 g; Mass of O = 23.2 g (total mass) - 16.8 g = 6.4 g, which is (6.4 g) / (16 g/mol) = 0.4 mol of O.To find the empirical formula, divide each mole value by the smallest number of moles: C=1.2/0.4, H=2.4/0.4, O=0.4/0.4, giving a ratio of C: 3 H: 6 O: 1. Therefore, the empirical formula is C3H6O.

Final answer:

Vitreous silica and soda-lime glass are distinct types of glass: vitreous silica has a low coefficient of expansion and excellent thermal stability, while soda-lime glass is more common, clearer, and easier to shape but has higher thermal expansion and less resistance to heat.

Explanation:

Differences Between Vitreous Silica and Soda-Lime Glass

Vitreous silica, commonly known as silica glass, and soda-lime glass are two prominent forms of glass with distinct properties and uses. Vitreous silica, which is composed predominantly of silicon dioxide (SiO2), has the valuable property of being highly transparent to both visible and ultraviolet light. The useful characteristics of vitreous silica also include a very low coefficient of expansion, which prevents it from fracturing during rapid temperature changes, making it ideal for items that undergo extreme temperature shifts, such as certain optical instruments and CorningWare.

On the other hand, soda-lime glass is a more common glass type, consisting of about 70 to 74% silica by weight mixed with sodium oxide, lime, and small amounts of other compounds such as magnesia and alumina. This type of glass is widely used for window panes, tableware, and containers, attributed to its clarity and ease of formation. Despite its widespread use, soda-lime glass does exhibit a high thermal expansion and is more prone to heat damage compared to silica glass.

Advantages and Disadvantages

Silica Glass:

Advantage: Excellent thermal stability and resistance to rapid temperature changes.

Disadvantage: More difficult to melt and shape, which may limit its use in some applications.

Soda-Lime Glass:

Advantage: Transparent and easily formed, suitable for everyday glass items.

Disadvantage: High thermal expansion and lower resistance to heat, making it less suitable for certain conditions.

Answer:the same as the ionization energy trend but opposite the atomic radius trend

Explanation:

Electron affinity refers to the ability of an atom to accept electrons and form a negative ion. This ability increases across the period but decreases down the group. The atomic radius of elements decrease across the period as more nuclear charge is added without a corresponding increase in the number of shells. As size of the nuclear charge increases, the ionization also increases. Down the group, the addition of more shells increases the distance of the outermost electron from the nucleus hence ionization energy decreases and atomic size increases. Electron affinity has the same trend as ionization energy but an opposite trend to atomic radius hence the answer.

The electron affinity trend is B. the same as the ionization energy trend but opposite the atomic radius trend.

Electron affinity simply means the ability of an atom to be able to accept electrons and then form a negative ion. It should be noted that an electron affinity trend increases across the period but decreases down the group.

On the other hand, the atomic radius of elements will decrease across the period when there are more nuclear charges that are added without a corresponding increase in the number of shells. Therefore, as the size of the nuclear charge increases, the ionization also increases.

In conclusion, the electron affinity trend is the same as the ionization energy trend but opposite the atomic radius trend.

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The pressure in the flask after the reaction is complete is approximately 1.84 atm, calculated using the Ideal Gas Law.

This question applies the Ideal Gas Law. The balanced chemical reaction is 2SO2 + O2 → 2SO3. So, for every 2 moles of SO2, 1 mole of O2 is required and 2 moles of SO3 are produced. Given that the moles of SO2 and O2 both are 0.20 mol, all the SO2 and half of O2 will react to form 0.20 mol of SO3 leaving only 0.10 mol of O2 unreacted in the flask. Therefore, the total number of moles of gases in the flask after reaction is 0.20 mol SO3 + 0.10 mol O2 = 0.30 mol. Applying the Ideal Gas Law: Pressure (P) = nRT/V, where n = total no. of moles = 0.30 mol,R = universal gas constant = 0.0821 L·atm/(mol·K),T = temperature in Kelvin = 25ºC + 273.15 = 298.15 K, V = volume = 4.0 L. After substituting these values in the formula, we calculate the pressure to be roughly 1.84 atm.

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After reacting 0.20 mol each of SO2 and O2 to form SO3 in a 4.0 L flask at 25°C, the pressure in the flask would be 2.46 atm.

The question presented involves the application of the Ideal Gas Law and stoichiometric relations in chemistry. Given that we have 0.20 mol of SO2 and 0.20 mol of O2 that react to form SO3, the first step is to use the balanced equation of the reaction: 2SO₂(g) + O₂(g) → 2SO₃(g). In this reaction, the total moles of gas would remain unchanged before and after the reaction. Therefore, the total number of moles of gas in the flask after the reaction would still be 0.20 + 0.20 = 0.40 mol.

Using the Ideal Gas Law PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant (0.0821 L·atm/mol·K), and T is temperature in Kelvin (25°C = 298K), we can calculate the pressure. Plugging in the given values: P = nRT/V = (0.4 mol)(0.0821 L.atm/mol.K)(298 K) / 4.0 L = 2.46 atm. Thus the pressure in the flask after the reaction is complete would be 2.46 atm.

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Answer:

C3H6

Explanation:

We can obtain the molecular formula by using the empirical formula and the molar mass in combination.

This is shown below:

[CH2]n = 42g/mol

We then add the atomic masses of carbon and hydrogen and multiply by n to give the value of n .

n[12 + 2(1)] = 42

14n = 42

n = 42/14 = 3

The molecular formula is thus [CH2]3 = C3H6

Answer:

C3H6

Explanation:

42g/mol=molar mass

14g/mol= emperical mass

42/14=3

3 times emperical

Answer: 0,4278g of F and 0,4191g of Fe

Explanation: it's possible to calculate the mass of each element by multiplying the percentage (decimal) of the element by the mass of the compound.

For Fluorine (F)

0,847g * 0,5051 = 0,4278g of F

For iron (Fe)

0,847 * 0,4949 = 0,4191g of Fe

This is determined because even when the compound is decomposed, due to conservative law of mass, the decomposition process do not affect the amount of matter, so the mass of the elements remain even if they are separated from the original molecule.

At the end, the sum of the elements masses should be the total mass of the compound.

Answer:fluorine=0.5082

Iron=0.3388

Explanation:

Using Empirical formula to show the ratio.

F. Fe

50.51/39 49.49/56

=1.295. 0.88375

=1.295/0.88375 :0.88375/0.88375

=1.465:1

multiply each term by 2 to get a whole number ratio,we have

=(1.465*2) :(1*2)

=2.93:2

=3:2

To get the amount if each contribution of F and Fe,we use ratio,

F=3/(3+2)=3/5*total mass(0.847)

F=0.5082g

Similarly,Fe=2/5*0.847

Fe=0.3388g.

Answer:

The answer to your question is 8.67 grams of Al₂O₃

Explanation:

Data

mass of Al₂O₃ = ?

mass of Al = 4.6 g

mass of O₂ = excess

Balanced Reaction

                   4Al   +    3O₂     ⇒    2Al₂O₃

            Reactants           Elements           Products

                    4                     Al                          4

                    6                      O                         6

Process

1.- Use proportions to calculate the moles of Al

                         27 g of Al ------------------  1 mol

                         4.6 g of Al ------------------  x

                           x = 0.17 mol of Al

2.- use proportions to calculate the moles of Al₂O₃

                   4 moles of Al ------------------  2 moles of Al₂O₃

                   0.17 moles of Al --------------  x

                        x = 0.085 moles of Al₂O₃

3.- Use proportions to calculate the grams of Al₂O₃

molecular mass Al₂O₃ = (27 x 2) + (16 x 3) = 102 g

                     102 g of Al₂O₃ ---------------  1 mol

                       x                     --------------- 0.085 moles

                       x = 8.67 g of Al₂O₃

The question is incomplete, here is the complete question:

Burning a compound of calcium, carbon, and nitrogen in oxygen in a combustion train generates calcium oxide (CaO), carbon dioxide [tex](CO_2)[/tex], nitrogen dioxide [tex](NO_2)[/tex], and no other substances. A small sample gives 2.389 g CaO, 1.876 g [tex]CO_2[/tex], and 3.921 g [tex]NO_2[/tex] Determine the empirical formula of the compound.

Answer: The empirical formula for the given compound is [tex]CaCN_2[/tex]

Explanation:

The chemical equation for the combustion of compound having calcium, carbon and nitrogen follows:

[tex]Ca_xC_yN_z+O_2\rightarrow CaO+CO_2+NO_2[/tex]

where, 'x', 'y' and 'z' are the subscripts of calcium, carbon and nitrogen respectively.

We are given:

Mass of CaO = 2.389 g

Mass of [tex]CO_2=1.876g[/tex]

Mass of [tex]NO_2=3.921g[/tex]

We know that:

Molar mass of calcium oxide = 56 g/mol

Molar mass of carbon dioxide = 44 g/mol

Molar mass of nitrogen dioxide = 46 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 1.876 g of carbon dioxide, [tex]\frac{12}{44}\times 1.876=0.5116g[/tex] of carbon will be contained.

For calculating the mass of nitrogen:

In 46 g of nitrogen dioxide, 14 g of nitrogen is contained.

So, in 3.921 g of nitrogen dioxide, [tex]\frac{14}{46}\times 3.921=1.193g[/tex] of nitrogen will be contained.

For calculating the mass of calcium:

In 56 g of calcium oxide, 40 g of calcium is contained.

So, in 2.389 g of calcium oxide, [tex]\frac{40}{56}\times 2.389=1.706g[/tex] of calcium will be contained.

To formulate the empirical formula, we need to follow some steps:

Moles of Calcium =[tex]\frac{\text{Given mass of Calcium}}{\text{Molar mass of Calcium}}=\frac{1.706g}{40g/mole}=0.0426moles[/tex]

Moles of Carbon =[tex]\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.5116g}{12g/mole}=0.0426moles[/tex]

Moles of Nitrogen = [tex]\frac{\text{Given mass of Nitrogen}}{\text{Molar mass of Nitrogen}}=\frac{1.193g}{14g/mole}=0.0852moles[/tex]

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0426 moles.

For Calcium = [tex]\frac{0.0426}{0.0426}=1[/tex]

For Carbon = [tex]\frac{0.0426}{0.0426}=1[/tex]

For Nitrogen = [tex]\frac{0.0852}{0.0426}=2[/tex]

The ratio of Ca : C : N = 1 : 1 : 2

Hence, the empirical formula for the given compound is [tex]CaCN_2[/tex]

The empirical formula of the compound containing calcium, carbon, and nitrogen is CaC2N.

The empirical formula of a compound can be determined from the ratio of the elements present in the compound. In this case, we need to find the smallest whole-number ratio of calcium, carbon, and nitrogen in the compound. From the given information, we know that there is 1 calcium, 2 carbon, and 1 nitrogen in the compound. To find the empirical formula, divide each count by the smallest count, which is 1 in this case. Therefore, the empirical formula of the compound is CaC2N.

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Answer:

23 kPa = Partial pressure O₂

Explanation:

In a mixture of gases, the sum of partial pressure of each gas that contains the mixture = Total pressure

Total pressure = Partial pressure N₂ + Partial pressure CO₂ + Partial pressure O₂

95 kPa = 48 kPa + 24 kPa + Partial pressure O₂

95 kPa - 48 kPa - 24 kPa = Partial pressure O₂

23 kPa = Partial pressure O₂

Final answer:

Given that 3.5 g of NO₂ is emitted in 10 minutes, over 40 minutes, an engine would release approximately 0.304 moles of NO₂, assuming emissions are consistent.

Explanation:

The question involves calculating the amount of NO₂ emitted from an automobile engine in moles over a specified period. Given that 3.5 g of NO₂ was emitted in 10 minutes, we can find the total amount emitted over a 40-minute period by setting up a proportion, as the emission is consistent under all circumstances. To find the number of moles, we use the molar mass of NO₂, which is approximately 46.01 g/mol.

First, calculate the total emitted mass over 40 minutes:

Then, calculate the number of moles of NO₂:

Therefore, if the engine were used for a 40-minute commute, it would release approximately 0.304 moles of NO₂, assuming steady emissions.

Answer:

Molarity of acid, Ca = Cb*Vb*A/Va*B

Explanation:

Using H2SO4 as acid, the reaction is as follow:

2NaOH  +  H2SO4 ⇒ Na2SO4  +  2H2O

Volume of acid = Va; Volume of base = Vb, Molar concentration of  acid = Ca; Molar concentration of base = Cb; Molarity of acid = A and Molarity of base = B

Ca*Va/Cb*Vb =A/B

∴ Ca = Cb*Vb*A/Va*B

Answer:

9 atm is the total pressure of the combined gases.

Explanation:

According to the Dalton's law of partial pressure , the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.

[tex]P_T=p_{1}+p_{2}....p_{n}[/tex]

where,

[tex]P_T[/tex] = total pressure =

[tex]p_{1}[/tex] = partial pressure of gas-1

[tex]p_{2}[/tex] = partial pressure of gas -2

[tex]p_{n}[/tex] = partial pressure of nth gas

We have :

Pressure of the oxygen gas in flask before mixing = 8 atm

Pressure of the hydrogen gas in flask before mixing = 1 atm

Partial pressure of oxygen gas after mixing = [tex]p_1=8 atm[/tex]

Partial pressure of hydrogen gas after mixing = [tex]p_2=1 atm[/tex]

Total pressure of the mixture : P

[tex]P=P_1+P_2[/tex] (Dalton's law of partial pressure)

[tex]P=8 atm+1 atm=9 atm[/tex]

9 atm is the total pressure of the combined gases.

Answer:

D

Explanation:

Answer:The stoichiometric coefficient for cobalt (Co) is 1.

Explanation:

To balance the chemical equation for the reaction between aluminum metal (Al) and aqueous cobalt(II) nitrate [Co(NO3)2], you need to ensure that the number of atoms of each element is the same on both sides of the equation. The given reaction can be written as follows:

Al + Co(NO3)2 → Al(NO3)3 + Co

Now, let's balance the equation:

Balance the aluminum (Al) atoms:

There is 1 Al atom on the left and 1 Al atom on the right. Aluminum is already balanced.

Balance the cobalt (Co) atoms:

There is 1 Co atom on the left, but 1 Co atom on the right. Cobalt is already balanced.

Balance the nitrogen (N) atoms:

There are 2 nitrate ions (NO3-) on the left and 3 nitrate ions on the right (since there are three nitrate ions in Al(NO3)3). To balance the nitrogen atoms, we need to put a coefficient of 3 in front of Co(NO3)2 on the left:

Al + 3Co(NO3)2 → Al(NO3)3 + Co

Now, the nitrogen atoms are balanced.

Balance the oxygen (O) atoms:

On the left, there are 3 nitrate ions, which contribute 3 x 3 = 9 oxygen atoms. On the right, there are 3 nitrate ions and 3 oxygen atoms in Al(NO3)3, which contribute a total of 3 x 3 + 3 = 12 oxygen atoms. To balance the oxygen atoms, we need to put a coefficient of 3 in front of Al(NO3)3 on the right:

Al + 3Co(NO3)2 → 3Al(NO3)3 + Co

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Final answer:

The balanced chemical equation for the formation of magnesium hydroxide and hydrogen from magnesium and water is Mg (s) + 2 H2O (l) → Mg(OH)2 (s) + H2 (g), with several possible mole ratios based on the equation's stoichiometry.

Explanation:

The equation for the formation of magnesium hydroxide and hydrogen gas from magnesium and water is:

Mg (s) + 2 H2O (l) → Mg(OH)2 (s) + H2 (g)

This reaction is balanced as written, with one atom of magnesium reacting with two molecules of water to produce one molecule of magnesium hydroxide and one molecule of hydrogen gas.

The possible mole ratios in this reaction are:

1 mole of Mg to 2 moles of H2O

1 mole of Mg to 1 mole of Mg(OH)2

1 mole of Mg to 1 mole of H2

2 moles of H2O to 1 mole of Mg(OH)2

2 moles of H2O to 1 mole of H2

These mole ratios are derived from the coefficients of each substance in the balanced chemical equation.

Answer:

230

Explanation:

The company declared 15% stock dividend, each share holder will receive an increment of 15 shares per 100 shares, since Hona owns 200 shares she will receive 30 more shares so that her total share will 230

Answer:0.026ml

Explanation:

Details are found in the image attached. We must subtract the saturated vapour pressure of hydrogen gas at the given temperature from the total pressure of the hydrogen gas collected over water to obtain the actual pressure of hydrogen gas and substitute the value obtained into the general gas equation. The dry hydrogen gas has no saturated vapour pressure hence the value is substituted as given. All temperatures must be converted to Kelvin before substitution.

To calculate the rate constant (k) at 75°C, we need the frequency factor (A) for the reaction, which is not provided in the question.

The rate constant (k) of a reaction can be calculated using the Arrhenius equation:

k = Ae-Ea/RT

where A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.

To calculate k at 75°C, we need to find the frequency factor (A) for the reaction. Unfortunately, the question does not provide the value of A, so we cannot calculate the rate constant at 75°C.

The rate constant ( k ) at 75°C is approximately [tex]\( {2.57 \times 10^{-5} \text{ s}^{-1}} \).[/tex]

To find the rate constant ( k ) at 75°C for a reaction with an activation energy given at 25°C, we'll use the Arrhenius equation. The Arrhenius equation relates the rate constant ( k ) to temperature ( T ) and the activation energy [tex]\( E_a \):[/tex]

[tex]\[ k = A \cdot e^{-\frac{E_a}{RT}} \][/tex]

Given data:

Step-by-Step Solution:

1. Convert activation energy to Joules per mole:

[tex]\[ E_a = 33.6 \times 10^3 \text{ J/mol} \][/tex]

2. Calculate ( k ) at 25°C (298.15 K):

First, express the Arrhenius equation in terms of [tex]\( k_{25} \)[/tex] and solve for ( A ):

[tex]\[ k_{25} = A \cdot e^{-\frac{E_a}{RT_{25}}} \][/tex]

[tex]\[ A = k_{25} \cdot e^{\frac{E_a}{RT_{25}}} \][/tex]

Calculate ( A ):

[tex]\[ A = 4.7 \times 10^{-3} \text{ s}^{-1} \cdot e^{\frac{33.6 \times 10^3 \text{ J/mol}}{8.314 \text{ J/(mol·K)} \cdot 298.15 \text{ K}}} \][/tex]

[tex]\[ A \approx 4.7 \times 10^{-3} \text{ s}^{-1} \cdot 6.55 \times 10^5 \][/tex]

[tex]\[ A \approx 3.08 \text{ s}^{-1} \][/tex]

3. Calculate ( k ) at 75°C (348.15 K):

Now use the calculated ( A ) and the new temperature [tex]\( T_{75} = 348.15 \) K:[/tex]

[tex]\[ k_{75} = A \cdot e^{-\frac{E_a}{RT_{75}}} \][/tex]

[tex]\[ k_{75} = 3.08 \text{ s}^{-1} \cdot e^{-\frac{33.6 \times 10^3 \text{ J/mol}}{8.314 \text{ J/(mol·K)} \cdot 348.15 \text{ K}}} \][/tex]

[tex]\[ k_{75} = 3.08 \text{ s}^{-1} \cdot e^{-11.51} \][/tex]

[tex]\[ k_{75} = 3.08 \text{ s}^{-1} \cdot 8.35 \times 10^{-6} \][/tex]

[tex]\[ k_{75} \approx 2.57 \times 10^{-5} \text{ s}^{-1} \][/tex]

Answer:

1.63425 × 10^- 18 Joules.

Explanation:

We are able to solve this kind of problem, all thanks to Bohr's Model atom. With the model we can calculate the energy required to move the electron of the hydrogen atom from the 1s to the 2s orbital.

We will be using the formula in the equation (1) below;

Energy, E(n) = - Z^2 × R(H) × [1/n^2]. -------------------------------------------------(1).

Where R(H) is the Rydberg's constant having a value of 2.179 × 10^-18 Joules and Z is the atomic number= 1 for hydrogen.

Since the Electrons moved in the hydrogen atom from the 1s to the 2s orbital,then we have;

∆E= - R(H) × [1/nf^2 - 1/ni^2 ].

Where nf = 2 = final level= higher orbital, ni= initial level= lower orbital.

Therefore, ∆E= - 2.179 × 10^-18 Joules× [ 1/2^2 - 1/1^2].

= -2.179 × 10^-18 Joules × (0.25 - 1).

= - 2.179 × 10^-18 × (- 0.75).

= 1.63425 × 10^- 18 Joules.

Answer:

The answer to your question is below

Explanation:

Factors that affect the rate of a chemical reaction

- Temperature        If the temperature increases the rate of reaction increases.

- Concentration     The reaction will move where there less concentration it could be to the reactants of products.

- Particle size         The lower the particle size the higher the rate of reaction.

- Catalyst                 Catalyzers accelerate the rate of reaction

- Pressure                The reaction will move where there are fewer molecules.

Final answer:

The rate of a chemical reaction is affected by the chemical nature of reactants, surface area, temperature, concentration, and the presence of a catalyst.

Explanation:

Factors Affecting the Rate of Chemical Reactions

The rate at which a chemical reaction proceeds can be influenced by various factors. Primary among these are the chemical nature of the reactants, the surface area, the temperature of the system, the concentration of reactants, and the presence of a catalyst. The chemical nature determines how reactive a substance is. The surface area comes into play particularly when reactants are in different phases; smaller particles or greater surface area contact typically speeds up reactions. Increasing the temperature usually causes reaction rates to increase because reactant molecules move faster and collide more often with enough energy to surmount the activation energy barrier. Similarly, higher reactant concentrations lead to more frequent collisions and a higher reaction rate. Lastly, a catalyst can provide an alternative reaction pathway with a lower activation energy, thus increasing the reaction rate without being consumed in the process.

Answer: speed of vibration = 146.33m/s

Explanation: The speed of sound (v) in a string is related to tension (T) and mass per unit length (u) via the formula

v = √T/u

T = 621N, m =32.4g = 0.0324kg, l= 1.12m

u = mass / length, thus

u = 0.0324/ 1.12 = 0.029kg/m

Hence

v = √621/ 0.028

v = √ 21,413.793

v = 146.33m/s

Answer:

1. Inversely proportional

2. Option C. Boyle's Law

3. Directly proportional

4. Option C. Gay-Lussac's Law

5. Directly proportional

6. Option C. Charles' Law

Explanation

Boyle's law states that the volume of a fixed mass of gas is inversely proportional to the pressure provided temperature remains constant. Mathematically,

V & 1/P

V = K/P

PV = K(constant)

Charles' law states that the volume of a fixed mass of gas is directly proportional to it's absolute temperature, provided pressure remains constant. Mathematically,

V & T

V = KT

V / T = K(constant)

Gay-Lussac's Law states that the pressure of a fixed mass of gas is directly proportional to it's absolute temperature, provided the volume remains constant. Mathematically

P & T

P = KT

P/ T = K (constant)

Answer: C

Explanation:

Pesticide, a substance used for destroying insects or other organisms harmful to cultivated plants or to animals.

Answer:

Answer: C

Explanation:

Pesticide, a substance used for destroying insects or other organisms harmful to cultivated plants or to a

Answer:

The answer to this question is 3.  Kinetic energy decreases as temperature decreases.

Explanation:

The average Kinetic energy is given by

[tex]K = \frac{3}{2}[/tex] × [tex]K_{B}[/tex] × T where

K = The average molecular kinetic energy of the gas (J)

[tex]K_{B}[/tex] = Boltzmann's constant (1.38×[tex]10^{-23}[/tex] J/K)

T = Temperature of the gas in Kelvin (k)

When the temperature of a given mass of gas drops average kinetic energy of the molecules goes down and the average molecular speed decreases.  The lower kinetic energy  which is the energy of motion of the molecules indicates lower speed of the molecules.

Note that, the kinetic energy and average speed are related by the following formula

KE = [tex]\frac{1}{2}[/tex]×m×v²

Where KE = Kinetic energy in Joules (J)

v = the velocity in m/s and

m = the mass of the molecule in Kg

Answer:

Answer is C

Explanation:

Edge 2020

Answer:

They tend to have the amide nitrogen protonated to give a positive charge.

Explanation:

A peptide bond joins two consecutive amino acids in the protein. The peptide bond is present between -CO group (also known as carboxyl group) of one amino acid and -NH2 group (also known as amino group) of another amino acid. It is represented as -CONH bond. Therefore, it is an amide linkage. The peptide bond always has planar orientation with trans configuration.  

Trans configuration avoids steric hindrance and hence, add to stability of the peptide bond.  

Nitrogen atom of peptide bond never bear positive charge

Therefore, the incorrect statement is as follows:

They tend to have the amide nitrogen protonated to give a positive charge.

Answer :

(a) Orange juice  → Heterogeneous mixture

(b) Tap water  → Homogeneous mixture

Explanation:

Homogeneous mixture:

It is a type of mixture in which the components of the mixture are distributed uniformly throughout the mixture.

It can not be separated by physically. It has only one phase.

Heterogeneous mixture:

It is a type of mixture in which all the components are completely mixed and the particles present in the mixture can be separated by physically.

They have two or more phase.

From the given options, tap water is a homogeneous mixture because it has only one phase.

While the other options, orange juice are heterogeneous mixture because it can be separated by physically and they have two or more phase.

Tap water is a homogeneous mixture because its composition is uniformly distributed and it appears as one substance. Orange juice, especially if it contains pulp, is a heterogeneous mixture since its components (pulp and liquid) are distinct and not uniformly mixed.

The substances in question, orange juice and tap water, can be classified as either homogeneous or heterogeneous mixtures. In a homogeneous mixture, the components are evenly mixed throughout and you can't see the different parts. Tap water is an example of this because it usually contains many different substances dissolved inside it like minerals, and gasses, but it still retains the same properties throughout, meaning it looks like one substance.

On the other hand, a heterogeneous mixture contains components that aren't evenly mixed and you can see the different parts. Orange juice, especially if it's freshly squeezed and contains pulp, is an example of a heterogeneous mixture. The pulp and liquid are very different in terms of texture and appearance and they don't blend into a single, indistinguishable mixture.

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The average rate of the reaction between 20 and 30 seconds is 0.012 M/s.

To calculate the average rate, we need to know the change in concentration of the reactant (A) and the time interval over which the change occurred. In this case, the change in concentration of A is 0.012 M (from 0.06 M to 0.048 M) and the time interval is 10 seconds (from 20 seconds to 30 seconds).

The average rate of the reaction is calculated as follows:

Average rate = Change in concentration / Time interval

= (0.012 M) / (10 s)

= 0.012 M/s

Therefore, the average rate of the reaction between 20 and 30 seconds is 0.012 M/s.

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The complete question is:

This graph shows the concentration of the reactant Ain the reaction A→B. Determine the average rate of the reaction between 20 and 30 seconds.

Answer:

2

Explanation:

A careful look at CO2, reveals that CO2 contains:

1 atom of C

2 atoms of O.

Answer:

2

Explanation:

i just took the test

Answer : The rate law for the overall reaction is, [tex]Rate=k[NO]^2[H_2][/tex]

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

As we are given the mechanism for the reaction :

Step 1 : [tex]2NO+H_2\rightarrow N_2+H_2O_2[/tex]    (slow)

Step 2 : [tex]H_2O_2+H_2\rightarrow 2H_2O[/tex]     (fast)

Overall reaction : [tex]2NO+2H_2\rightarrow N_2+2H_2O[/tex]

The rate law expression for overall reaction should be in terms of [tex]NO\text{ and }H_2[/tex].

As we know that the slow step is the rate determining step. So,

The slow step reaction is,

[tex]2NO+H_2\rightarrow N_2+H_2O_2[/tex]

The expression of rate law for this reaction will be,

[tex]Rate=k[NO]^2[H_2][/tex]

Hence, the rate law for the overall reaction is, [tex]Rate=k[NO]^2[H_2][/tex]

Answer :

(a) The balanced molecular equation will be,

[tex]3KSCN(aq)+Fe(NO_3)_3(aq)\rightarrow Fe(SCN)_3(aq)+3KNO_3(aq)[/tex]

(b) The complete ionic equation in separated aqueous solution will be,

[tex]3K^+(aq)+3SCN^{-}(aq)+Fe^{3+}(aq)+NO_3^{-}(aq)\rightarrow Fe^{3+}(aq)+3SCN^{-}(aq)+3K^+(aq)+3NO_3^-(aq)[/tex]

(c) In this equation the all the species are in aqueous state. So, there is no net ionic form of the reaction.

Explanation :

Complete ionic equation : In complete ionic equation, all the substance that are strong electrolyte and present in an aqueous are represented in the form of ions.

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

(a) The balanced molecular equation will be,

[tex]3KSCN(aq)+Fe(NO_3)_3(aq)\rightarrow Fe(SCN)_3(aq)+3KNO_3(aq)[/tex]

(b) The complete ionic equation in separated aqueous solution will be,

[tex]3K^+(aq)+3SCN^{-}(aq)+Fe^{3+}(aq)+NO_3^{-}(aq)\rightarrow Fe^{3+}(aq)+3SCN^{-}(aq)+3K^+(aq)+3NO_3^-(aq)[/tex]

(c) In this equation the all the species are in aqueous state. So, there is no net ionic form of the reaction.

The student's question involves the reaction between Fe(NO₃)₃ and KSCN forming FeSCN²⁺ and KNO₃. This explanation includes the molecular, complete ionic, and net ionic forms of the equation, with further context on the effect of KNO₃ on the reaction equilibrium.

To answer the student's question, we need to write equations for the reaction between aqueous Fe(NO₃)₃ (Iron(III) nitrate) and aqueous KSCN (potassium thiocyanate) to form aqueous FeSCN²⁺ (Iron(III) thiocyanate) and aqueous KNO₃ (potassium nitrate). Here is the breakdown:

Fe(NO₃)₃(aq) + 3 KSCN(aq) → Fe(SCN)₃(aq) + 3 KNO₃(aq)

Fe³⁺(aq) + 3 NO₃⁻(aq) + 3 K⁺(aq) + 3 SCN⁻(aq) → Fe(SCN)₃²⁺(aq) + 3 K⁺(aq) + 3 NO₃⁻(aq)

Fe³⁺(aq) + 3 SCN⁻(aq) → Fe(SCN)₃²⁺(aq)

In this experiment, the presence of Fe(SCN)²⁺ is indicated by a color change, but adding KNO₃, according to Le Chatelier's principle, will shift the equilibrium left, reducing Fe(SCN)²⁺ concentration.

Answer:

a. the K+ ions are attracted to the partial negative charge on the oxygen atom of the water molecule.

Explanation:

The hydrogen atoms on water are partially positive and the oxygen on water is partially negative.

Since unlike charges attract, the oxygen of the water molecules are attracted to the K+ and the hydrogens are attracted to Cl-.  the water surrounds the k+ and cl- so that the unlike charges are allowed to be close together.

The proper response to KCl dissolving in water is e. the Cl- ions are attracted to dissolved K+ ions.

The ionic compound KCl separates into the ions K+ and Cl- when it is introduced to water. The partial negative charges on the oxygen atoms in the water molecules are what draw the positive K+ ions to them. At the same time, the partial positive charges on the hydrogen atoms of the water molecules draw the negative Cl- ions towards them. Ion-dipole interactions are the name for this attraction between ions and water molecules.

In the case of KCl, the dissolved K+ ions in the solution selectively attract the Cl- ions. Due to the polar nature of the individual ions, the water molecules form a hydration shell around them.

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