Question

6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles...

6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles of CH4, and 0.590 moles of CCl4 are at equilibrium in a 17.7 L container at 576 K, the value of the equilibrium constant, Kc, is

6B)Consider the following reaction:

COCl2(g) CO(g) + Cl2(g)

If 3.59×10-3 moles of COCl2, 0.265 moles of CO, and 0.211 moles of Cl2 are at equilibrium in a 12.3 L container at 772 K, the value of the equilibrium constant, Kp, is

Homework Answers

Answer #1

A)

[CH2Cl2] = number of mol of CH2Cl2 / volume in L

= 0.432 mol / 17.7 L

= 0.0244 M

[CH4] = number of mol of CH4 / volume in L

= 0.263 mol / 17.7 L

= 0.0149 M

[CCl4] = number of mol of CCl4 / volume in L

= 0.590 mol / 17.7 L

= 0.0333 M

Now use:

Kc = [CH4][CCl4] / [CH2Cl2]^2

= (0.0149 * 0.0333) / (0.0244)^2

= 0.833

Answer: 0.833

B)

for COCl2:

Given:

V = 12.3 L

n = 3.59e-3 mol

T = 772.0 K

use:

P * V = n*R*T

P * 12.3 L = 0.0036 mol* 0.08206 atm.L/mol.K * 772 K

P = 0.0185 atm

for CO:

Given:

V = 12.3 L

n = 0.265 mol

T = 772.0 K

use:

P * V = n*R*T

P * 12.3 L = 0.265 mol* 0.08206 atm.L/mol.K * 772 K

P = 1.3649 atm

for Cl2:

Given:

V = 12.3 L

n = 0.211 mol

T = 772.0 K

use:

P * V = n*R*T

P * 12.3 L = 0.211 mol* 0.08206 atm.L/mol.K * 772 K

P = 1.0867 atm

Now use:

Kp = p(Cl2)*p(CO)/p(COCl2)

= (1.0867 * 1.3649)/ (0.0185)

= 80.2

Answer: 80.2

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.09E-2 M CH2Cl2, 0.165 M CH4 and 0.165 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.82E-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CCl4] = M The equilibrium constant, K,...
A. The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)<---> CH4(g)...
A. The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)<---> CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.346 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. B. The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g) <---> 2 CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.200 moles of CH4and 0.200 moles of CCl4are introduced into a...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.19×10-2 M CH2Cl2, 0.168 M CH4 and 0.168 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.133 mol of CH4(g) is added to the flask? [CH2Cl2] =____ M [CH4] = ______M [CCl4] = ______M
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.856 atm at 350 K. PCH2Cl2 = ________ atm PCH4 = _________ atm PCCl4 = _______ atm
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K. CH4 (g) +...
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K. CH4 (g) + CCl4 (g) <-> 2 CH2Cl2 (g) Calculate the equilibrium concentrations of reactants and product when 0.281 moles of CH4 and 0.281 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] = [CCl4] = [CH2Cl2] =
The equilibrium constant, Kp, for the following reaction is 9.52×10-2 at 350 K: CH4(g) + CCl4(g)...
The equilibrium constant, Kp, for the following reaction is 9.52×10-2 at 350 K: CH4(g) + CCl4(g) 2CH2Cl2(g) Calculate the equilibrium partial pressures of all species when CH4 and CCl4, each at an intitial partial pressure of 1.12 atm, are introduced into an evacuated vessel at 350 K. PCH4 = ________ atm PCCl4 = ________atm PCH2Cl2 = ________ atm
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.276 moles of CO and 0.276 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = ___M [Cl2] = ___M [COCl2] = ___M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.306 moles of CO and 0.306 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
The equlibrium constant K, for the following reaction is 2.00 x 10-2 at 613 K. COCl2(g)...
The equlibrium constant K, for the following reaction is 2.00 x 10-2 at 613 K. COCl2(g) CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 18.4 L container at 613 K contains 0.194 M COCl2, 6.22 x 10-2 M CO and 6.22 x10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 7.62 L? [COCl2]= _____________M [CO]=____________M...
-Consider the following reaction: 2HI(g) H2(g) + I2(g) If 3.69 moles of HI(g), 0.570 moles of...
-Consider the following reaction: 2HI(g) H2(g) + I2(g) If 3.69 moles of HI(g), 0.570 moles of H2, and 0.558 moles of I2 are at equilibrium in a 16.6 L container at 818 K, the value of the equilibrium constant, Kc, is_____________ .Consider the following reaction: 2NH3(g) N2(g) + 3H2(g) If 1.31×10-3 moles of NH3(g), 0.681 moles of N2, and 0.495 moles of H2 are at equilibrium in a 18.6 L container at 893 K, the value of the equilibrium constant,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT