A solution is composed of 1.90 mol cyclohexane (P°=97.6 torr) and 2.60 mol acetone (P°=229.5 torr). What is the mole fraction of cyclohexane in the vapor?

Final answer:

a) The ratio of lb-mole O2 react/lb-mole NO formed is 1.25. b) The oxygen feed rate corresponding to 40% excess O2 is 175.0 kmol/h. c) Ammonia is the limiting reactant, with the oxygen being in excess by 5.85%. The extent of reaction is 36.17 mol NO produced, with a mass of 1085.73 g.

Explanation:

a. To calculate the ratio (lb-mole O2 react/lb-mole NO formed), we can use the stoichiometry of the reaction. From the balanced equation, we can see that for every 5 moles of O2, we get 4 moles of NO. So, the ratio is 5/4 or 1.25 lb-moles O2 react/lb-mole NO formed.

b. To find the oxygen feed rate corresponding to 40% excess O2, we need to calculate the stoichiometric amount of O2 required and then add 40% of that amount. Since the reaction requires 5 moles of O2 for every 4 moles of NO, the stoichiometric amount of O2 required is (5/4) * 100.0 kmol NH3/h = 125.0 kmol O2/h. Adding 40% of that amount gives 125.0 kmol O2/h + (40/100) * 125.0 kmol O2/h = 175.0 kmol O2/h.

c. To determine the limiting reactant, we need to compare the amounts of ammonia and oxygen given. The molecular weight of ammonia (NH3) is 17 g/mol and oxygen (O2) is 32 g/mol. So, the mass of 50.0 kg of ammonia is 50.0 kg * (1000 g/kg) / (17 g/mol) = 2941.18 mol. The mass of 100.0 kg of oxygen is 100.0 kg * (1000 g/kg) / (32 g/mol) = 3125.0 mol. Comparing these amounts, we can see that ammonia is the limiting reactant as there is less of it. The percentage by which the other reactant (oxygen) is in excess can be calculated as [(3125.0 mol - 2941.18 mol) / 3125.0 mol] * 100 = 5.85 %. The extent of reaction and mass of NO produced can be determined using the stoichiometry of the reaction. From the balanced equation, we can see that for every 4 moles of NO produced, 5 moles of O2 are consumed. So, the extent of reaction is (3125.0 mol - 2941.18 mol) / 5 = 36.17 mol NO produced. The mass of NO produced can be calculated as 36.17 mol * (30.01 g/mol) = 1085.73 g.

a) Ratio (lb-mole O2 react/lb-mole NO formed) is 1.25 lb-mole O₂ / lb-mole NO.

b) Oxygen feed rate is 175.0 kmol O₂/h.

c) Limiting reactant is NH₃; Percentage excess of O₂ is 10.1%; Extent of reaction is 2.94 kmol NH₃; Mass of NO produced is 88.23 kg

a. Calculate the ratio (lb-mole O₂ react/lb-mole NO formed).

b. If ammonia is fed to a continuous reactor at a rate of 100.0 kmol NH₃/h, what oxygen feed rate (kmol/h) would correspond to 40.0% excess O₂?

c. If 50.0 kg of ammonia and 100.0 kg of oxygen are fed to a batch reactor, determine the limiting reactant, the percentage by which the other reactant is in excess, and the extent of reaction and mass of NO produced (kg) if the reaction proceeds to completion.

Explanation:

The sped of sound is given as follows.

            C = [tex]\sqrt{\gamma RT}[/tex]

It is known that for hydrogen,

         R = 4124 J/kg K

         T = 288 k

       [tex]\gamma[/tex] = 1.41

Therefore, calculate the value of [tex]C_{hydrogen}[/tex] as follows.

         [tex]C_{hydrogen} = \sqrt{\gamma RT}[/tex]

                     = [tex]\sqrt{1.41 \times 4124 J/kg K \times 288}[/tex]

                     = 1294.1 m/s

For helium,

         R = 2077 J/kg K

         T = 288 k

       [tex]\gamma[/tex] = 1.66

Therefore, calculate the value of [tex]C_{helium}[/tex] as follows.

         [tex]C_{helium} = \sqrt{\gamma RT}[/tex]

                     = [tex]\sqrt{1.66 \times 2077 J/kg K \times 288}[/tex]

                     = 996.48 m/s

For nitrogen,

         R = 296.8 J/kg K

         T = 288 k

       [tex]\gamma[/tex] = 1.4

Therefore, calculate the value of [tex]C_{hydrogen}[/tex] as follows.

         [tex]C_{hydrogen} = \sqrt{\gamma RT}[/tex]

                     = [tex]\sqrt{1.4 \times 296.8 J/kg K \times 288}[/tex]

                     = 345.93 m/s

So, speed of sound in hydrogen is calculated as follows.

            = [tex]\sqrt{1.41 \times 4124 \times T_{H}}[/tex]

            = [tex]76.26 \sqrt{T_{H}}[/tex]

Speed of sound in helium is as follows.

            = [tex]\sqrt{1.66 \times 2077 \times T_{He}}[/tex]

            = [tex]58.72 \sqrt{T_{He}}[/tex]

For both the speeds to be equal,

       [tex]76.26 \sqrt{T_{H}}[/tex] = [tex]58.72 \sqrt{T_{He}}[/tex]

        [tex]\frac{T_{H}}{T_{He}}[/tex] = 0.593

Therefore, we can conclude that the temperature of hydrogen is 0.593 times the temperature of helium.

Answer:

The average pressure in the container due to these 75 gas molecules is [tex]P=9.72 \times 10^{-16} Pa[/tex]

Explanation:

Here Pressure in a container is given as

[tex]P=\frac{1}{3} \rho <u^2>[/tex]

Here

                                         [tex]\rho =\frac{mass}{Volume of container}[/tex]

        Here

                mass is to be calculated for 75 gas phase molecules as

                      [tex]m=n_{molecules} \times \frac{1 mol}{6.022 \times 10^{23} molecules} \times \frac{32 g/mol}{1 mol}\\m=75 \times \frac{1 mol}{6.022 \times 10^{23} molecules} \times \frac{32 g/mol}{1 mol}\\m=3.98 \times 10^{-21} g[/tex]

              Volume of container is 0.5 lts

     So density is given as

                         [tex]\rho =\frac{mass}{Volume of container}\\\rho =\frac{3.98 \times 10^{-21} \times 10^{-3} kg}{0.5 \times 10^{-3} m^3}\\\rho =7.97 \times 10^{-21}\, kg/m^3[/tex]

                                        [tex]<u^2>=RMS^2[/tex]

      Here RMS is the Root Mean Square speed given as 605 m/s so

                                      [tex]<u^2>=RMS^2\\<u^2>=(605)^2\\<u^2>=366025[/tex]

Substituting the values in the equation and solving

[tex]P=\frac{1}{3} \rho <u^2>\\P=\frac{1}{3} \times 7.97 \times 10^{-21} \times 366025\\P=9.72 \times 10^{-16} Pa[/tex]

So the average pressure in the container due to these 75 gas molecules is [tex]P=9.72 \times 10^{-16} Pa[/tex]

Explanation:

(a)   The given data is as follows.

           Speed of electron (u) = [tex]5.5 \times 10^{4} m/s[/tex]

According to De Broglie's formula,

                wavelength, [tex]\lambda = \frac{h}{mu}[/tex]

where,   h = Planck's constant = [tex]6.626 \times 10^{-34} Js[/tex]

              m = mass of electron = [tex]9.11 \times 10^{-31} kg[/tex]

Hence, we will calculate the wavelength as follows.

           [tex]\lambda = \frac{h}{mu}[/tex]

                      = [tex]\frac{6.626 \times 10^{-34}}{9.11 \times 10^{-31}kg \times 5.5 \times 10^{4} m/s}[/tex]

                      = [tex]0.132 \times 10^{-7}[/tex] m

                      = [tex]13.2 \times 10^{-9}[/tex] m

It is known that for any microscope, smallest object that can be observed is equal to [tex]\frac{1}{2}[/tex] the wavelength of of the radiation  smallest object observable with an electron microscope.

Hence,     [tex]\frac{13.2 \times 10^{-9}}{2}[/tex]

                = [tex]6.6 \times 10^{-9}[/tex] m

               = 6.6 nm          (as 1 m = [tex]10^{-9} nm[/tex])

Therefore, the smallest object observable with an electron microscope will be 6.6 nm.

(b)  At [tex]3.0 \times 10^{7} m/s[/tex], the wavelength will be calculated as follows.

              wavelength, [tex]\lambda = \frac{h}{mu}[/tex]

                                  = [tex]\frac{6.626 \times 10^{-34} Js}{9.11 \times 10^{-31} kg \times 3.0 \times 10^{7} m/s}[/tex]

                                  = [tex]24.2 \times 10^{-12}[/tex] m

As, for any microscope, smallest object that can be observed is equal to [tex]\frac{1}{2}[/tex] the wavelength of of the radiation  smallest object observable with an electron microscope.

                = [tex]\frac{24.2 \times 10^{-12}}{2}[/tex]

                = [tex]12.1 \times 10^{-12} m \times 10^{9}nm/m[/tex]

                = 0.0121 nm

Therefore, at [tex]3.0 \times 10^{7} m/s[/tex]  the smallest object observable with an electron microscope is 0.0121 nm.

The smallest object observable with an electron microscope can be calculated using the formula: Size of object = Wavelength of electrons / 2. Plugging in the values and solving for the size of the object gives: Size of object = 3.37 x 10^-12 m. For a speed of 3.0 x 10^7 m/s, the calculation would be: Size of object = 1.22 x 10^-10 m.

The smallest object observable with an electron microscope can be calculated using the formula:

Size of object = Wavelength of electrons / 2

Using the given speed of 5.5 x 10^4 m/s, we can calculate:

Size of object = (h / (m * v)) / 2, where h is Planck's constant and m is the mass of an electron.

Plugging in the values and solving for the size of the object gives:

Size of object = (6.626 x 10^-34 J s / (9.109 x 10^-31 kg * 5.5 x 10^4 m/s)) / 2

Size of object = 3.37 x 10^-12 m

For a speed of 3.0 x 10^7 m/s, the calculation would be:

Size of object = (6.626 x 10^-34 J s / (9.109 x 10^-31 kg * 3.0 x 10^7 m/s)) / 2

Size of object = 1.22 x 10^-10 m

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Answer:

Explanation:

a ) Speed of radio waves in space = speed of light in space

= 3 x 10⁸ m /s

Time taken = distance / speed

= 8.1 x 10⁷ x 10³ / 3 x 10⁸ s

= 2.7 x 10² s

= 270 s

b )

Distance = speed x time

= 3 x 10⁸ x 1.2 m

= 3.6 x 10⁸ m

= 3.6 x 10⁵ km

Answer:

a) Yes, these bands of signals overlap.

b) FM has broader transmission band.

Explanation:

a) Frequency range of TV channels = 59.5 to 215.8 MHz

Wavelength range of FM radio = 2.78 m to 3.41 m

Frequency of the wave = [tex]\nu [/tex]

Wavelength of the wave = [tex]\lambda [/tex]

Speed of light = c = [tex]3\times 10^8 m/s[/tex]

[tex]\nu =\frac{c}{\lambda }[/tex]

Frequency of wave with, [tex]\lambda = 2.78 m[/tex]

[tex]\nu =\frac{3\times 10^8 m/s}{2.78 m}=1.079\times 10^8 Hz[/tex]

[tex]1.079\times 10^8 Hz=1.079\times 10^8\times 10^{-6} MHz=107.9 MHz[/tex]

Frequency of wave with, [tex]\lambda = 3.41m[/tex]

[tex]\nu =\frac{3\times 10^8 m/s}{3.41 m}=8.798\times 10^7 Hz[/tex]

[tex]8.798\times 10^7 Hz=8.798\times 10^7\times 10^{-6} MHz=87.98 MHz[/tex]

Frequency range of FM = 87.89 to 107.9 MHz

Frequency range of TV channels = 59.5 to 215.8 MHz

Yes, these bands of signals overlap.

b)  

Frequency range of AM = 550 to 1600 kHz

1 kHz = 0.001 MHz

550 to 1600 kHz = [tex]550\times 0.001 MHz[/tex] to [tex]1600\times 0.001 MHz[/tex]

= 0.55 MHz to 1.6 MHz

Frequency range of AM = 0.55 to 1.6 MHz

Frequency range of FM = 87.89 to 107.9 MHz

FM has broader transmission band.

The question is incomplete, here is the complete question:

371. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.118 atm at 25°C. Calculate the molar mass of the protein. Round your answer to 3 significant digits.

Answer: The molar mass of the unknown protein is [tex]1.54\times 10^3g/mol[/tex]

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

[tex]\pi=iMRT[/tex]

or,

[tex]\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT[/tex]

where,

[tex]\pi[/tex] = osmotic pressure of the solution = 0.118 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of protein = 371. mg = 0.371 g   (Conversion factor:  1 g = 1000 mg)

Molar mass of protein = ?

Volume of solution = 5.00 mL

R = Gas constant = [tex]0.0821\text{ L atm }mol^{-1}K^{-1}[/tex]

T = temperature of the solution = [tex]25^oC=[25+273]K=298K[/tex]

Putting values in above equation, we get:

[tex]0.118atm=1\times \frac{0.371\times 1000}{\text{Molar mass of protein}\times 5}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 298K\\\\\pi=\frac{1\times 0.371\times 1000\times 0.0821\times 298}{0.118\times 5}=1538.4g/mol=1.54\times 10^3g/mol[/tex]

Hence, the molar mass of the unknown protein is [tex]1.54\times 10^3g/mol[/tex]

The molarity of the solution when 23.640 g of Mn(ClO4)2 · 6 H2O is added to 200.0 mL of water is 0.3014 M, calculated by dividing the moles of solute by the volume of solution in liters.

To calculate the molarity of a solution when a certain amount of solute is added to a known volume of water, you must first determine the number of moles of solute. For the molarity of the resulting solution when 23.640 g of Mn(ClO4)2 · 6 H2O (molar mass approximately 392.13 g/mol) is dissolved in 200.0 mL of water, the calculation is as follows:

To calculate the moles of Mn(ClO4)2 · 6 H2O: 23.640 g / 392.13 g/mol ≈ 0.06028 mol.

To find molarity (M), which is moles of solute per liter of solution: 0.06028 mol / 0.200 L = 0.3014 M.

Answer: The osmotic pressure of the solution is 3.29 atm

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

[tex]\pi=iMRT[/tex]

or,

[tex]\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT[/tex]

where,

[tex]\pi[/tex] = osmotic pressure of the solution = ?

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of sucrose = 12.8 grams

Molar mass of sucrose = 342.3 g/mol

Volume of solution = 278 mL

R = Gas constant = [tex]0.082\text{ L atm }mol^{-1}K^{-1}[/tex]

T = temperature of the solution = 298 K

Putting values in above equation, we get:

[tex]\pi=1\times \frac{12.8\times 1000}{342.3\times 278}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 298K\\\\\pi=3.29atm[/tex]

Hence, the osmotic pressure of the solution is 3.29 atm

Answer: aldehyde

Explanation:

the aldehyde group (—CHO) is always at the extreme

The question is incomplete, here is the complete question:

Consider the following multistep reaction:

C+D⇌CD (fast)

CD+D→CD₂ (slow)

CD₂+D→CD₃ (fast)

C+3D→CD₃

Based on this mechanism, determine the rate law for the overall reaction.

Answer: The rate law for the reaction is [tex]\text{Rate}=k'[C][D]^2[/tex]

Explanation:

Rate law is the expression which is used to express the rate of the reaction in terms of the molar concentration of reactants where each term is raised to the power their stoichiometric coefficient respectively from a balanced chemical equation.

In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.

For the given chemical reaction:

[tex]C+3D\rightarrow CD_3[/tex]

The intermediate reaction of the mechanism follows:

Step 1:  [tex]C+D\rightleftharpoons CD;\text{ (fast)}[/tex]

Step 2:  [tex]CD+D\rightarrow CD_2;\text{(slow)}[/tex]

Step 3:  [tex]CD_2+D\rightarrow CD_3;\text{(fast)}[/tex]

As, step 2 is the slow step. It is the rate determining step

Rate law for the reaction follows:

[tex]\text{Rate}=k[CD][D][/tex]           ......(1)

As, [CD] is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.

Applying steady state approximation for CD from step 1, we get:

[tex]K=\frac{[CD]}{[C][D]}[/tex]

[tex][CD]=K[C][D][/tex]

Putting the value of [CD] in equation 1, we get:

[tex]\text{Rate}=k.K[C][D]^2\\\\\text{Rate}=k'[C][D]^2[/tex]  

Hence, the rate law for the reaction is [tex]\text{Rate}=k'[C][D]^2[/tex]

Answer:

g = 1.11x10⁻⁵Ω.

Explanation:

The membrane conductance (g) can be calculated by dividing membrane current (I) through the driving force (Vm - E) as follows:  

[tex] g_{ion} = \frac{I_{ion}}{V_{m} - E_{ion}} [/tex]

where Vm: is the membrane potential and [tex]E_{ion}[/tex]: is the equilibrium potential for the ion or reversal potential.  

The equilibrium potential for the ion can be calculated using the Nernst equation:

[tex] E_{ion} = \frac{RT}{zF}*Ln(\frac{[ion]_{out}}{[ion]_{ins}}) [/tex]

where R: is the gas constant = 8.314 J/K*mol, F: is the Faraday constant = 96500 C/mol, T: is the temperature (K), z: is the ion's charge, [ion]out and [ion]ins: is the concentration of the ion outside and inside, respectively.    

[tex] E_{ion} = \frac{(8.314 J*K^{-1}*mol^{-1})((15 + 273)K)}{(+1)(96500 C*mol^{-1})}*Ln(\frac{[500mM]}{[70mM]}) = 48.78 mV [/tex]  

Now, we can calculate the  membrane conductance (g) using equation (1):

[tex] g_{ion} = \frac{I_{ion}}{V_{m} - E_{ion}} = \frac{-318*10^{-9} A}{20*10^{-3} V - 48.78*10^{-3} V} = 1.11*10^{-5} \Omega [/tex]

Therefore, the membrane conductance is 1.11x10⁻⁵Ω.

I hope it helps you!        

Answer: 10 ml of 200 mM [tex]CaCl_2[/tex] is required and 30 ml of water is required.

Explanation:

According to the dilution law,

[tex]C_1V_1=C_2V_2[/tex]

where,

[tex]C_1[/tex] = concentration of stock solution = 200mM

[tex]V_1[/tex] = volume of stock solution = ?

[tex]C_2[/tex] = concentration of resulting solution= 50mM

[tex]V_2[/tex] = volume of another acid solution= 40 ml

[tex]200\times x=50\times 40[/tex]

[tex]x=10ml[/tex]

Thus 10 ml of 200 mM [tex]CaCl_2[/tex] is required and (40-10) ml = 30 ml of water is to be added to make 40 ml of 50mM [tex]CaCl_2[/tex].

Final answer:

To make 40 ml of a 50 mM CaCl2 solution from a 200 mM stock, you need 10 ml of the stock solution and 30 ml of water.

Explanation:

To calculate how much of the 200 mM CaCl2 stock solution you need to dilute to get 40 ml of a 50 mM solution, you can use the dilution formula C1V1 = C2V2, where C1 is the concentration of the stock solution, V1 is the volume of the stock solution needed, C2 is the final concentration, and V2 is the final volume. Plugging in the known values yields (200 mM) × V1 = (50 mM) × (40 ml), solving for V1 gives V1 = (50 mM × 40 ml) / (200 mM) = 10 ml. Therefore, to make 40 ml of a 50 mM CaCl2 solution, you need 10 ml of the 200 mM stock and to dilute it with 30 ml of water.

Statements 1 is correct.

Explanation:

Pentanal - is an aldehyde have the molecular formula C₅H₁₀O, is soluble in organic solvent and it is derived from Pentane.

3-pentanone is a ketone have the molecular formula C₅H₁₀O.

1,3,5-pentanetriol is an alcohol have the molecular formula C₅H₁₂O₃.

All the 3 molecules have 5 carbon atoms and they don't have equal number of hydrogen atoms.

Pentanal and pentanone, both have carbonyl groups.

3-pentanone is slightly soluble in water, whereas 1,3,5-pentanetriol is mostly soluble in water, since it contains 3-OH groups forms hydrogen bond with water.

All three molecules are derived from Pentane and not from Pentyne.

So statement 1 is correct.

Answer:

For a: The edge length of the unit cell is 314 pm

For b: The radius of the molybdenum atom is 135.9 pm

Explanation:

To calculate the edge length for given density of metal, we use the equation:

[tex]\rho=\frac{Z\times M}{N_{A}\times a^{3}}[/tex]

where,

[tex]\rho[/tex] = density = [tex]10.28g/cm^3[/tex]

Z = number of atom in unit cell = 2  (BCC)

M = atomic mass of metal (molybdenum) = 95.94 g/mol

[tex]N_{A}[/tex] = Avogadro's number = [tex]6.022\times 10^{23}[/tex]

a = edge length of unit cell =?

Putting values in above equation, we get:

[tex]10.28=\frac{2\times 95.94}{6.022\times 10^{23}\times (a)^3}\\\\a^3=\frac{2\times 95.94}{6.022\times 10^{23}\times 10.28}=3.099\times 10^{-23}\\\\a=\sqrt[3]{3.099\times 10^{-23}}=3.14\times 10^{-8}cm=314pm[/tex]

Conversion factor used:  [tex]1cm=10^{10}pm[/tex]  

Hence, the edge length of the unit cell is 314 pm

To calculate the edge length, we use the relation between the radius and edge length for BCC lattice:

[tex]R=\frac{\sqrt{3}a}{4}[/tex]

where,

R = radius of the lattice = ?

a = edge length = 314 pm

Putting values in above equation, we get:

[tex]R=\frac{\sqrt{3}\times 314}{4}=135.9pm[/tex]

Hence, the radius of the molybdenum atom is 135.9 pm

Answer:

A. 47 protons and 58 neutrons, 47 protons and 64 neutrons

B. 47 electrons

Explanation:

While it is possible for two isotopes of a particular element to have different atomic masses, it is. It is impossible for the number of protons or the atomic number of the isotopes to be different.

To answer this question properly, we would be needing the proton number or the atomic number of silver. The atomic number of silver is 47. Let’s say the isotopes are A and B respectively.

The number of protons in the same is equal which is 47. The number of neutrons is different and can be obtained by subtracting the number of protons from the mass number.

For A: neutrons = 105 - 47 = 58

For B: neutrons = 111 - 47 = 64

Since Both are electrically neutral, the number of orbiting electrons is also equals the number of protons which is equal to 47.

Silver (Ag) has 47 protons. Its isotopes Ag-105 and Ag-111 have 58 and 64 neutrons respectively. In neutral conditions both isotopes have 47 electrons.

The atomic number for silver (Ag) is 47, which means it has 47 protons. Isotopes of a particular element have the same number of protons but different number of neutrons. Isotope Ag-105 will have 47 protons and 105 - 47 = 58 neutrons, and Isotope Ag-111 will have 47 protons and 111 - 47 = 64 neutrons. In a state of electrical neutrality (no charge), an atom will have the same number of protons and electrons. Thus, both Isotopes Ag-105 and Ag-111 will each have 47 electrons.

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To determine the final temperature after ice is dropped into water, we analyze the energy transfer phases: ice warming, melting, and temperature equalization, applying specific heat capacities and latent heat of fusion.

To find the final temperature after dropping a cube of ice into water, we must consider the energy exchanges that occur: the ice warming up to 0°C, melting, and the resulting water warming up or cooling down to reach thermal equilibrium with the water already in the glass. For this, we use the concept of specific heat capacity and the latent heat of fusion for water.

The specific heat capacity of ice is about 2.062 J/(g°C), and the specific heat capacity of liquid water is 4.184 J/(g°C). The latent heat of fusion of ice is roughly 334 J/g. By applying the conservation of energy, we equate the heat lost by the warmer substance (water) to the heat gained by the colder substance (ice and the water resulting from melted ice), taking into account phase changes.

However, without numerical calculation in this particular example, the key takeaway is understanding the phases of energy transfer: warming up the ice, melting the ice, and then equalizing the temperature of the mixture. The initial temperatures of the substances and their masses play crucial roles in determining the final temperature.

Answer:

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Explanation:

the complete explanation is found in the attachment

A subsidy from the water district to local plant nurseries would lower the cost of production, enabling them to offer more drought-tolerant plants. This would shift the supply curve to the right on a graph, representing an increase in supply. Assuming demand remains steady, this could result in a lower price and increased quantity of plants.

In the economics of supply and demand, a subsidy given to local plant nurseries would likely increase the supply of drought-tolerant plants like purple sage. As the cost of production decreases due to the subsidy, nurseries can afford to produce and sell more plants, shifting the supply curve to the right.

On a graph showing supply and demand curves, you would drag the supply curve to the right to represent this change. This movement should ideally cause a decrease in the price of the plants and increase in quantity, assuming demand stays consistent.

This scenario illustrates the basic economic principle that if you reduce the cost of production (in this case by providing a subsidy), producers are able to supply more of the product, leading to increases in quantity and potential decreases in price. This is an effective tool used often by governments and organizations to influence market dynamics and promote specific goods or services.

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Answer:

The percentage yield of methanol is 78.74%.

Explanation:

[tex]2H_2+CO\rightarrow CH_3OH[/tex]

Theoretical yield of methanol ;

Moles of hydrogen gas = [tex]\frac{5.0 g}{2 g/mol}=2.5 mol[/tex]

Moles of carbon monoxide = [tex]\frac{5.0 g}{28 g/mol}=0.1786 mol[/tex]

According to reaction ,1 mole of CO reacts with 2 moles of hydrogen gas. Then 0.1786 moles of CO will :

[tex]\frac{2}{1}\times 0.1786 mol=0.0893 mol[/tex]

As we can see, that moles of hydrogen gas are in excess and CO are in limiting amount, so amount of methanol will depend upon moles of CO.

According to recation 1 mole of CO gives 1 mole of methanol, then 0.1786 moles of CO will give:

[tex]\frac{1}{1}\times 0.1786 mol=0.1786 mol[/tex]

Mass of 0.1786 moles of methanol =

= 0.1786 mol × 32 g/mol = 5.7152 g

Theoretical yield of methanol  = 5.7152 g

Experimental yield of methanol = 4.5 g

Percentage yield of methanol:

To calculate the percentage yield , we use the equation:

[tex]\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100[/tex]

[tex]=\frac{4.5 g}{5.7152 g}\times 100=78.74\%[/tex]

The percentage yield of methanol is 78.74%.

The percent yield of the reaction is approximately 78.53%.

First, we need to write the balanced chemical equation for the reaction between hydrogen [tex](H_2)[/tex] and carbon monoxide (CO) to produce methanol [tex](CH_3OH)[/tex]:

[tex]\[ 2H_2 + CO \rightarrow CH_3OH \][/tex]

From the stoichiometry of the balanced equation, we can see that 2 moles of hydrogen react with 1 mole of carbon monoxide to produce 1 mole of methanol.

Now, we calculate the moles of hydrogen and carbon monoxide that reacted:

Molar mass of hydrogen [tex](H_2)[/tex] = 2 [tex]\times[/tex] 1.008 g/mol = 2.016 g/mol

Moles of hydrogen = mass / molar mass = 5.0 g / 2.016 g/mol = 2.48 moles

Molar mass of carbon monoxide (CO) = 12.01 g/mol + 16.00 g/mol = 28.01 g/mol

Moles of carbon monoxide = mass / molar mass = 5.0 g / 28.01 g/mol = 0.179 moles

Since the reaction requires a 2:1 ratio of hydrogen to carbon monoxide, and we have fewer moles of carbon monoxide, carbon monoxide is the limiting reactant.

The balanced equation tells us that 1 mole of CO produces 1 mole of methanol. Therefore, the theoretical yield of methanol is equal to the moles of CO that reacted:

Theoretical yield in moles = 0.179 moles

Now, we convert the moles of methanol to grams using its molar mass:

Molar mass of methanol [tex](CH_3OH)[/tex] = 12.01 g/mol (C) + 4 \times 1.008 g/mol (H) + 16.00 g/mol (O) = 32.042 g/mol

Theoretical yield in grams = theoretical yield in moles \times molar mass = 0.179 moles \times 32.042 g/mol = 5.73 g

The actual yield of the reaction is given as 4.5 g of methanol.

Now, we can calculate the percent yield:

[tex]\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \][/tex]

[tex]\[ \text{Percent Yield} = \left( \frac{4.5 \text{ g}}{5.73 \text{ g}} \right) \times 100\% \][/tex]

[tex]\[ \text{Percent Yield} \approx 78.53\% \][/tex]

Answer:

[tex]\lambda=2.61\times 10^{-9}\ m[/tex] = 261 nm

Silver is not a good choice.

Explanation:

[tex]E=\frac {h\times c}{\lambda}[/tex]

Where,  

h is Plank's constant having value [tex]6.626\times 10^{-34}\ Js[/tex]

c is the speed of light having value [tex]3\times 10^8\ m/s[/tex]

[tex]\lambda[/tex] is the wavelength of the light

Given that:- Energy = [tex]7.59\times 10^{-19}\ J[/tex]

[tex]7.59\times 10^{-19}=\frac{6.626\times 10^{-34}\times 3\times 10^8}{\lambda}[/tex]

[tex]7.59\times \:10^{26}\times \lambda=1.99\times 10^{20}[/tex]

[tex]\lambda=2.61\times 10^{-9}\ m[/tex] = 261 nm

Visible range has a spectrum of 380 to 740 nm

So, Silver is not a good choice.

The maximum wavelength needed to remove an electron from silver is approximately 262 nm. Silver is not a good choice for a photocell that uses visible light.

To find the maximum wavelength needed to remove an electron from silver, we can use the work function of silver, which is Φ = 4.73 eV. The threshold wavelength for observing the photoelectric effect in silver can be calculated using Equation 6.16, which is λ = hc/Φ. Substituting the given values, we have λ = (1240 eV⋅nm) / (4.73 eV), which gives us a threshold wavelength of approximately 262 nm. Since visible light ranges from 400 to 700 nm, silver is not a good choice for a photocell that uses visible light.

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Answer:

1.067

Explanation:

Using the Arrhenius equation relates rate constants to the temperature is:

ln(k2/k1) = −Ea/R * [1/T2−1/T1]

where,

Ea = activation energy in kJ/mol ,

R = universal gas constant, and

T = temperature in K .

T1 = 25 + 273.15

= 298.15 K

T2 = 34 + 273.15

= 307.15 K

k1 = 0.816

Therefore,

k2/k1 = exp(-22.7/0.008314472) * [1/307.15 −1/298.15 ])

= 0.816 * 1.308

k2 = 1.067.

Answer:

moles sebacoyl chloride = 2.1 x 10-3 mol

Explanation:

Answer:

12.45

Explanation:

There is some info missing. I think this is the original question.

A chemist dissolves 169 mg of pure barium hydroxide in enough water to make up 70 mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 2 significant decimal places.

First, we will calculate the molarity of barium hydroxide.

M = mass / molar mass × liters of solution

M = 0.169 g / 171.34 g/mol × 0.070 L

M = 0.014 M

Barium hydroxide is a strong base that dissociates according to the following equation.

Ba(OH)₂ → Ba²⁺ + 2 OH⁻

The molar ratio of Ba(OH)₂ to OH⁻ is 1:2. The concentration of OH⁻ is 2 × 0.014 M = 0.028 M

The pOH is:

pOH = -log [OH⁻] = - log 0.028 = 1.55

The pH is:

pH = 14 - pOH = 14 - 1.55 = 12.45

Answer:

1. Co^2+ 1s2 2s2 2p6 3s2 3p6 3d7

2. N^3- 1s2 2s2 2p6

3. Ca^2+ 1s2 2s2 2p6 3s2 3p6

Explanation:

When Cobalt loses 2 electrons to become Co2+ it loses the electrons which are in 4s2, not the ones in 3d7 because the electrons in 4s2 have a high reactivity. Thus, when electrons are lost from Co atom, they are lost from the 4s orbital first because it is actually higher in energy when both 3d and 4s are filled with electrons.

Explanation:

a) IE1 of Germenium.  ionization energy decreases down the group.

b) Here IE2 of Ga is higher because second valence electron of gallium is in s orbital whereas second valence electron of germenium is in p orbital.

c) IE3 of Ge is higher as this follows the trend.

d)IE4 of Ga is higher because the 4th valence electron of Ga is a core electron and the for Ge it is in s orbital and it takes higher energy to break a core electron than the orbital ones.

When comparing Ga and Ge, IE₁ and IE₂ of Ga are lower due to being earlier in the periodic table, but IE₄ of Ga is expected to be higher as it involves removing an electron from a full orbital. IE₃ for both may be similar due to both elements having three valence electrons. The correct answer is d) IE₄ of Ga or IE₄ of Ge.

The subject in question involves comparing first and successive ionization energies (IE) for elements in the periodic table, particularly gallium (Ga) and germanium (Ge). Ionization energy refers to the energy required to remove an electron from a gaseous atom or ion.

As general rules, (a) the first IE tends to increase across a period as the nuclear charge increases, and (b) IE increases for successive ionizations as the atom or ion becomes progressively more positively charged.

(a) IE₁ of Ga would be lower than IE₁ of Ge because Ga is to the left of Ge in the periodic table, and thus Ge has a higher nuclear charge and a stronger attraction to its valence electron.

(b) IE₂ of Ga would also be lower than IE₂ of Ge because the additional electron from Ga would come from the same valence shell as the first electron, while Ge's second ionization would remove an electron that experiences a stronger nuclear charge.

(c) As both Ga and Ge have three valence electrons, the IE₃ of Ga and Ge will both involve removing an electron from a similarly charged ion, but because Ga has a higher energy 4p subshell, its IE₃ might be slightly lower than Ge's, which is removing an electron from the 4s subshell (which after removing two electrons is now full and lower in energy).

(d) At the IE₄ level, we see a large jump in ionization energy for both elements as electrons are being removed from an energy level closer to the nucleus; however, IE₄ of Ga will generally be higher than IE₄ of Ge due to  of an electron from a full orbital in Ga, which has higher energy compared to the removal from a half-filled orbital in Ge.

These comparisons are based on the understanding that ionization energies increase both with increasing positive charge and with the removal of electrons closer to the nucleus.

Answer: the volume of the sample decreased

Explanation:

T1 = -98°C = - 98 + 273 = 175K

T2 = -89°C = -89 +273 = 184K

P1 = P

P2 = 110%P = 1.1P

V1 = V

V2 =?

P1V1/T1 = P2V2/T2

PxV/175 = 1.1PxV2/184

175x1.1PxV2 = PVx 184

V2 = (PVx 184) /(175x1.1P)

V2 = 0.96V = 96%V

Therefore, the final volume is 96% of the initial volume. This means that the final volume decreased by 96%

The volume of the sample will increase.  

• Based on the given information,  

• Let us assume that we have constant number of moles of nitrogen gas at -98 degree C, and the initial pressure is P1.  

• It is given that the pressure is increased by 10%, and the temperature is increased to -89 degree C.  

Now, the final pressure (P2) will be,  

P1 + P1*10/100 = 1.10 P1

T1 = -98 degree C = -98 + 273 K = 175 K

T2 = -89 degree C = -89 + 273 K = 184 K

At constant no of moles, the ideal gas equation is,  

PV = nRT

Here, n and R are constant, So, P1V1/T1 = P2V2/T2

P1 * V1/T1 / 175 K = 1.10 P1 * V2/184K

V2/V1 = 184/175 * 1.10 = 1.15  

V2 = 1.15 V1

Thus, the volume of sample increase by 1.15 times from the initial volume.

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Answer:

293.99 g

OR

0.293 Kg

Explanation:

Given data:

Lattice energy of Potassium nitrate (KNO3) = -163.8 kcal/mol

Heat of hydration of KNO3 = -155.5 kcal/mol

Heat to absorb by KNO3 = 101kJ

To find:

Mass of KNO3 to dissolve in water = ?

Solution:

Heat of solution = Hydration energy - Lattice energy

                           = -155.5 -(-163.8)

                           = 8.3 kcal/mol

We already know,

1 kcal/mol = 4.184 kJ/mole

Therefore,

= 4.184 kJ/mol x 8.3 kcal/mol

= 34.73 kJ/mol

Now, 34.73 kJ of heat is absorbed when 1 mole of KNO3 is dissolved in water.

For 101 kJ of heat would be

= 101/34.73

= 2.908 moles of KNO3

Molar mass of KNO3 = 101.1 g/mole

Mass of KNO3 = Molar mass x moles

                         = 101.1 g/mole  x  2.908

                         = 293.99 g

                         = 0.293 kg

293.99 g potassium nitrate has to dissolve in water to absorb 101 kJ of heat.     

Final answer:

To absorb 101 kJ of heat, 7.63 grams of potassium nitrate must dissolve in water, calculated based on the lattice energy and heat of hydration provided.

Explanation:

The question asks how much potassium nitrate needs to dissolve in water to absorb 101 kJ of heat, given the lattice energy and heat of hydration for potassium nitrate. First, we convert the given heat into kcal because the energies are provided in kcal/mol: 101 kJ × (1 kcal / 4.184 kJ) = 24.1 kcal. The total heat involved in dissolving potassium nitrate in water can be found by adding the lattice energy to the heat of hydration: -163.8 kcal/mol + (-155.5 kcal/mol) = -319.3 kcal/mol. This value represents the heat released when 1 mole of potassium nitrate dissolves in water.

To find the amount of potassium nitrate that needs to dissolve to absorb 101 kJ (24.1 kcal), we set up a proportion, knowing that -319.3 kcal is released per mole of potassium nitrate dissolved: (1 mole / -319.3 kcal) = (x moles / 24.1 kcal). Solving for x gives x = 24.1 kcal / -319.3 kcal/mol = 0.0755 moles. Finally, to find the mass of potassium nitrate, we multiply the moles by the molar mass of potassium nitrate (KNO3), which is approximately 101.1 g/mol: 0.0755 moles ×101.1 g/mol = 7.63 grams.

Therefore, 7.63 grams of potassium nitrate need to dissolve in water to absorb 101 kJ of heat.

To calculate the concentration of the NaOH solution, convert the volume to grams and calculate the moles of NaOH. Then, use the moles and total volume to find the concentration.

To find the concentration of the NaOH solution, we need to calculate the moles of NaOH present in the 3.03 mL volume. First, we convert the volume to grams using the density of the solution: 3.03 mL × 1.53 g/mL = 4.6419 g

Next, we calculate the moles of NaOH:

Moles of NaOH = \dfrac{4.6419 g}{40.00 g/mol} = 0.1160 mol

Finally, we use the moles of NaOH and the total volume of the solution (500 mL) to find the concentration:

Concentration = \dfrac{0.1160 mol}{0.5000 L} = 0.2320 M

Final answer:

The concentration of the diluted NaOH solution after measuring 3.03 mL of a 50% NaOH solution, with a density of 1.53 g/mL, and diluting to 500 mL total volume is 0.1159 M.

Explanation:

To calculate the concentration of the diluted NaOH solution, we need to determine the amount of NaOH in the initial 3.03 mL of 50% solution and then find the molarity after dilution to 500 mL. The density of the solution is given as 1.53 g/mL, so the mass of the 3.03 mL solution is:

mass = volume × density = 3.03 mL × 1.53 g/mL = 4.6359 g

Since the solution is 50% by weight, the mass of NaOH is:

mass of NaOH = 0.50 × 4.6359 g = 2.3180 g

The molar mass of NaOH is approximately 40.00 g/mol, so the number of moles of NaOH in the original solution is:

moles of NaOH = mass / molar mass = 2.3180 g / 40.00 g/mol = 0.05795 mol

After dilution to 500 mL, the molarity (M) is calculated as follows:

Molarity = moles / volume (L) = 0.05795 mol / 0.50 L = 0.1159 M

Therefore, the concentration of the diluted NaOH solution is 0.1159 M.

Answer: Ms. Scarlet is the murderer.

Explanation: Each color has a wavelength band, some visible to the human eye (visible spectrum), some for the other animals. In this game of "Clue", the color are yellow (Col. Mustard), violet (Prof. Plum), green (Mr. Green), blue (Ms. Peacock) and red (Ms. Scarlet). Using the device and knowing each band, it's determined that at the time of murder, Mr. Green was in the dining room, because green light has the wavelength between 495 to 570nm; Prof. Plum was in the library, due to violet's light has the shortest wavelength; Col. Mustard and Ms. Peacock were either in the lounge or in the study, because of their color's light wavelength measurement. So, the person responsible for the murderer was Ms. Scarlet, as the other devices in the other places didn't register a higher wavelength, which is compatible to the red light.

According to the spectrometer readings, Ms. Peacock is the murderer of Ms. White in the conservatory, as the reflected colors in the other rooms correspond to the other characters' colors and leave only Ms. Peacock unaccounted for at the crime scene.

To determine who killed Ms. White in the conservatory in a game of "Clue" using a spectrometer, we need to match the color associated with the wavelength of light reflected in each room with the corresponding suspect's color. The dining room spectrometer recorded a reflection at 520 nm, which corresponds to green.

Since Mr. Green reflects green and that is his character color, he is in the dining room. The lounge and study recorded reflections of lower frequencies i.e., longer wavelengths than green, which suggest colors towards the red end of the spectrum, likely placing Ms. Scarlet (red) and Prof. Plum (purple) in those rooms.

The library recorded a reflection of the shortest possible wavelength, meaning violet, which is typically associated with Prof. Plum; however, since he is presumed to be in a room with a longer wavelength, that leaves Col. Mustard (who wears yellow) as the suspect in the library because yellow requires the absorption of wavelengths at the violet end of the spectrum.

Therefore, Ms. Peacock, whose color is blue and wasn't indicated in the other rooms, must have been in the conservatory and is determined to be the murderer according to the spectrometer readings.

Answer:

The new pH after adding HCl is 7.07

Explanation:

The formula for calculating pH of a buffer is

pH = pKa + log([Conjugate base]/[Acid])

Before adding HCl,

         7.55 = 7.55 + log([Conjugate base]/[Acid])

⇔      log([Conjugate base]/[Acid])  = 0

⇔     [Conjugate base] = [Acid] = 1/2 x 0.100 = 0.05 M

⇒ Mole of Conjugate base = Mole of Acid = 0.05 M x 0.12 mL = 0.006 mol

After adding HCl (3.00 mL, 1.00 M)

⇒ Mole of HCl = 0.003 x 1 = 0.003 mol)

New volume solution is 120 m L+ 3 mL = 123 mL

HCl is a strong acid, it will convert the conjugate base to acid form, or we can express

Mole of new Conjugate base = 0.006 - 0.003 = 0.003 mol

                ⇒ Concentration = 0.003/0.123 M

Mole of new Acid form = 0.006 + 0.003 = 0.009 mol

                ⇒ Concentration = 0.009/0.123 M

Use the formula

pH = pKa + log([Conjugate base]/[Acid])

    = 7.55 + log(0.003 / 0.009) = 7.07

To determine the new pH after adding HCl to the TES buffer, we need to consider the Henderson-Hasselbalch equation. Initially, the concentration of TES is 0.100 M and the pH is 7.55. After adding 3.00 mL of 1.00 M HCl, we need to calculate the new concentration of TES and its conjugate base. Using the Henderson-Hasselbalch equation, we can find the new pH by substituting the new concentration of TES, its conjugate base, and the pKa of TES into the equation.

To determine the new pH after adding HCl to the TES buffer, we need to consider the Henderson-Hasselbalch equation. The equation relates the pH of a buffer solution to the pKa of the acid and the ratio of the concentrations of the acid and its conjugate base. In this case, TES acts as the acid and its conjugate base is the salt.

The Henderson-Hasselbalch equation can be written as pH = pKa + log([A-]/[HA]), where [A-]/[HA] is the ratio of the salt to the acid. Initially, the concentration of TES is 0.100 M and the pH is 7.55. After adding 3.00 mL of 1.00 M HCl, we need to calculate the new concentration of TES and its conjugate base.

Using the equation c1V1 = c2V2, where c1 and V1 are the initial concentration and volume of HCl, and c2 and V2 are the final concentration and volume, we can find the new concentration of TES. The initial volume of TES is 120 mL. The final volume is the sum of the initial volume and the volume of HCl added. Calculate the new volume of TES from this information, and then substitute the values into the equation to find the new concentration of TES.

Once we have the new concentration of TES, we can use the Henderson-Hasselbalch equation to find the new pH. Substitute the new concentration of TES and the concentration of its conjugate base into the equation, along with the pKa of TES. Solve for the new pH to determine the answer.

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