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### For the reaction: 2H2O(g) ↔ 2H2(g) + O2(g)

What are the correct values of x, y, and z for the equilibrium expression to be correct?
Select one or more:

### Question 2

For the reaction: CO(g) + Cl2(g) ↔ COCl2(g)

What are the correct values of x, y, and z for the equilibrium expression to be correct?

Select one or more:

### Question 3

For the reaction: CO2(g) ↔ CO(g) + 0.5O2(g)

What are the correct values of x, y, and z for the equilibrium expression to be correct?

Select one or more:

f. y="1

### Question 4

For the reaction: Si(s) + O2(g) ↔ SiO2(s)

What are the correct values of x, y, and z for the equilibrium expression to be correct?

Select one or more:

### Question 5

At a certain temperature the equilbrium constant is 135 for

H2(g) + I2(g) ↔ 2HI(g)

Calculate the the equilbrium constant for

0.5H2(g) + 0.5I2(g) ↔ HI(g)

### Question 6

The equilbrium constant for the water-gas shift reaction is 5.0 at 400 oC:

CO(g) + H2O(g) ↔ CO2(g) + H2(g)

Determine Qc if the following amounts (in moles) of each component is placed in a 1.0 L container.

CO 0.53
H2O 0.27
CO2 0.89
H2 0.65

### Explanation

Keq= 5

Q= [CO2][H2]/[CO][H20]

Q=[0.89][0.65]/[0.53][0.27]= 4.04

### Question 7

What is the direction of the reaction for the above conditions?

Select one:

Q<Keq

goes to right

### Question 8

Determine Qc if the following amounts (in moles) of each component is placed in a 1.0 L container.

CO 0.34
H2O 0.11
CO2 0.88
H2 0.80

### Explanation

Q = [.88][.8]/[.11][.34]

=18.82

### Question 9

What is the direction of the reaction for the above conditions?

Select one:

Q>Keq

goes to the left

### Question 10

The equilbrium constant for the following reaction is 0.16 M0.5 at 3000 K:

CO2(g)  CO(g) + 0.5O2(g)

Determine Qc if the following amounts (in moles) of each component is placed in a 3.00 L container.

CO2 0.900
CO 0.840
O2 0.200

Give answer to 3 decimal places.

### Explanation

Remember to use concentration (mol/L)!!

Q= [O2]^.5[CO]/[CO2]

Q= (0.2/3)^.5(0.840/3)/(.900/3)

Q=.242

### Question 11

What is the direction of the reaction for the above conditions?

Select one:

Q> K

goes to the left

### Question 12

Determine Qc if the following amounts (in moles) of each component is placed in a 10.00 L container.

CO2 0.560
CO 0.260
O2 0.560

### Explanation

Q= [O2]^.5[CO]/[CO2]
Q= [.560/10]^.5[.260/10]/[.560/10]

Q=.11

### Question 13

What is the direction of the reaction for the above conditions?

Select one:

### Explanation

Q<Keq

goes to the right

### Question 14

Phosgene is formed from carbon monoxide and chlorine. At 607 oC, Kc is approximately 13.5 M-1 or L/mol. Calculate Kp (in atm-1) at this temperature.

CO(g) + Cl2(g) ↔ COCl2(g)

### Explanation

Kp = Kc (RT)^deltan

Kp= 13.5 (0.0821*(607-273.15)^1

Kp= .187

### Question 15

Some ammonia is sealed in a container and allowed to equilibrate at a particular temperature. The reaction is endothermic.

2NH3(g) ↔ N2(g) + 3H2(g)

In which direction will the reaction occur if some ammonia is removed from the system?

Select one:

### Question 16

In which direction will the reaction occur if some hydrogen is removed from the system?

Select one:

### Question 17

In which direction will the reaction occur if the volume of the container is decreased?

Select one:

### Question 18

In which direction will the reaction occur if the temperature is increased?

Select one:
-

### Question 19

In which direction will the reaction occur if argon is added to the system at constant volume. Thus, increasing the total pressure in the container?

Select one:

### Question 20

Chemists studied the formation of phosgene by sealing 0.76 atm of carbon monoxide and 1.14 atm of chlorine in a reactor at a certain temperature. The pressure dropped smoothly to 1.32 atm as the system reached equilbrium. Calculate Kp (in atm-1) for

CO(g) + Cl2(g) ↔ COCl2(g)

### Explanation

Hint, find the final pressure of each gas.

Use ICE Tables to solve:

CO Cl2 COCl2

I 0.76 1.14 0
C -x -x +x
E 0.76-x 1.14 -x x

1.32 = (0.76-x)+ (1.14-x)+x
Solve: -x=-0.58
x=0.58

CO Cl2 COCl2
I 0.76 1.14 0
C -0.58 -0.58 0.58
E 0.18 0.56 0.58

([0.58]/[0.18][0.56]) = 5.75

### Question 21

Consider 1.80 mol of carbon monoxide and 3.80 mol of chlorine sealed in a 4.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 for

CO(g) + Cl2(g) ↔ COCl2(g)

Calculate the equilibrium molar concentration of CO.

### Explanation

Hint, you need to find the equilibrium concentrations of all the gases. Note, that only one of the solutions to the quadratic equation makes sense (the other gives at least one negative concentration).

CO(g) + Cl2(g) ↔ COCl2(g)

I 1.8/4     3.8/4        0

C -x         -x           +x

E 1.8/4 -x   3.8/4 -x   x

Kc = 2.5 = x/ (1.8/4 -x)(3.8/4-x)

x=.2815

1.8/4 - .2815 = .1685