Question

A 1.0 L flask is charged with a gaseous mixture of 1.00 mol each of gaseous...

A 1.0 L flask is charged with a gaseous mixture of 1.00 mol each of gaseous reactants,CO, H2O, and 1.00 mol each of gaseous products CO2 and H2 and exposed to a zinc oxide - copper oxide catalyst at 500 K. Determine the composition of the mixture at equilibrium at this temperature.The equilibrium constant, Kc, atthis temperature is 102

Homework Answers

Answer #1

CO + H2O   -----------------------> CO2 + H2

1.0     1.0                                  1.0     1.0

1 - x    1-x                                   1+x    1+x

Kc = [CO2][H2] / [CO][H2O]

102 = (1+x)^2 / (1-x)^2

10.1 = 1+x / 1-x

x = 0.82

[CO] = [H2O] = 1 - x = 1 - 0.82 = 0.18 M

[CO2] = [H2] = 1 + x = 1 + 0.82 = 1.82 M

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
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O...
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g)+H2(g)⇌CO(g)+H2O(g) Calculate Kc for the reaction.
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container CO(g) + H2O(g) <===> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) <-----> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
A mixture of 0.2000 mol of CO2 , 0.1000 mol of H2 , and 0.1600 mol...
A mixture of 0.2000 mol of CO2 , 0.1000 mol of H2 , and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K : CO2(g)+H2(g)←−→CO(g)+H2O(g) Calculate the initial partial pressure of CO2 .         Calculate the initial partial pressure of H2 . Calculate the initial partial pressure of H2O . At equilibrium PH2O=3.51atm . Calculate the equilibrium partial pressure of CO2 .
Kc=102 at 500 K A reaction mixture initially contains 0.140M CO and 0.140M H2O Part A:...
Kc=102 at 500 K A reaction mixture initially contains 0.140M CO and 0.140M H2O Part A: What will be the equilibrium concentration of [CO]? Part B: What will be the equilibrium concentration of [H2O]? Part C: What will be the equilibrium concentration of [CO2]? Part D: What will be the equilibrium concentration of [H2]?
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M COand 0.120 M H2O. A)What will be the equilibrium concentration of [CO]? B)What will be the equilibrium concentration of [H2O]? C)What will be the equilibrium concentration of [CO2]? D)What will be the equilibrium concentration of [H2]?
A mixture of 0.01484 mol of H2O, 0.07019 mol of CH4, 0.01819 mol of CO, and...
A mixture of 0.01484 mol of H2O, 0.07019 mol of CH4, 0.01819 mol of CO, and 0.09015 mol of H2 is placed in a 1.0-L steel pressure vessel at 1239 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g)--> 1 CO(g) + 3 H2(g) At equilibrium 0.01097 mol of H2O is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = Peq(CH4) = Peq(CO) = . Peq(H2) = ....
An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) +H20 (g) --> <-- CO2 (g) + H2 (g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a...
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a certain temperature contains 26.8 g CO and 2.35 g H2. At equilibrium, the flask contains 8.64 g CH3OH. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. 2. Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1358 torr and a H2O partial pressure of 1764 torr at 2000 K....
When 1.10 mol CO2 and 1.10 mol H2 are placed in a 3.00-L container at 395...
When 1.10 mol CO2 and 1.10 mol H2 are placed in a 3.00-L container at 395 ∘C, the following reaction occurs: CO2(g)+H2(g)⇌CO(g)+H2O(g). A. If Kc = 0.802, what are the concentrations of CO2 in the equilibrium mixture?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT