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

Select one or more: f. y="1 g. y="2 h. z="0 i. z="1 j. z="2

For the reaction: CO(g) + Cl_{2}(g) ↔ COCl_{2}(g)

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

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

Select one or more:

For the reaction: CO_{2}(g) ↔ CO(g) + 0.5O_{2}(g)

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

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

Select one or more:

f. y="1

For the reaction: Si(s) + O_{2}(g) ↔ SiO_{2}(s)

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

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

Select one or more:

At a certain temperature the equilbrium constant is 135 for

H_{2}(g) + I_{2}(g) ↔ 2HI(g)

Calculate the the equilbrium constant for

0.5H_{2}(g) + 0.5I_{2}(g) ↔ HI(g)

H

Calculate the the equilbrium constant for

0.5H

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

CO(g) + H

Determine Q

CO 0.53

H

CO

H

Keq= 5

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

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

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

Select one:

Q<Keq

goes to right

Determine Q_{c} if the following amounts (in moles) of each component is placed in a 1.0 L container.

CO 0.34

H_{2}O 0.11

CO_{2} 0.88

H_{2} 0.80

CO 0.34

H

CO

H

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

=18.82

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

Select one:

Q>Keq

goes to the left

The equilbrium constant for the following reaction is 0.16 M^{0.5} at 3000 K:

**CO**_{2}(g) ↔** CO(g) + 0.5O**_{2}(g)

Determine Q_{c} if the following amounts (in moles) of each component is placed in a 3.00 L container.

CO_{2} 0.900

CO 0.840

O_{2} 0.200

Give answer to 3 decimal places.

Determine Q

CO

CO 0.840

O

Give answer to 3 decimal places.

Remember to use concentration (mol/L)!!

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

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

Q=.242

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

Select one:

Q> K

goes to the left

Determine Q_{c} if the following amounts (in moles) of each component is placed in a 10.00 L container.

CO_{2} 0.560

CO 0.260

O_{2} 0.560

CO

CO 0.260

O

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

Q= [.560/10]^.5[.260/10]/[.560/10]

Q=.11

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

Select one:

Q<Keq

goes to the right

Phosgene is formed from carbon monoxide and chlorine. At 607 ^{o}C, K_{c} is approximately 13.5 M^{-1} or L/mol. Calculate K_{p} (in atm^{-1}) at this temperature.

CO(g) + Cl_{2}(g) ↔ COCl_{2}(g)

CO(g) + Cl

Kp = Kc (RT)^deltan

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

Kp= .187

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

2NH_{3}(g) ↔ N_{2}(g) + 3H_{2}(g)

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

2NH

In which direction will the reaction occur if some ammonia is

Select one:

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

Select one:

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

Select one:

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

Select one:a. Left to right (more product)

-c. No change (reaction still at equilibrium)

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:

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 K_{p} (in atm^{-1}) for

CO(g) + Cl_{2}(g) ↔ COCl_{2}(g)

CO(g) + Cl

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

Consider 1.80 mol of carbon monoxide and 3.80 mol of chlorine sealed in a 4.00 L container at 476 ^{o}C. The equilibrium constant, K_{c}, is 2.50 for

CO(g) + Cl_{2}(g) ↔ COCl_{2}(g)

Calculate the equilibrium molar concentration of CO.

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) + Cl_{2}(g) ↔ COCl_{2}(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