Question 1

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g) ⇌ H2(g) + D2(g)  K = 0.28
2H2(g) + 2D2(g) ⇌ 4HD(g) K = ?

Accepted Answer

A)  7.8 × 10-2
B)  3.6
C)  0.53
D)  13
E)  1.9F) B) and E)
G) C) and D)

Question 2

For the following reaction, what is Δn required in the conversion of Kc to Kp? 2SO2(g) + O2(g) ⇌ 2SO3(g)

Accepted Answer

A)  3
B)  -1
C)  -2
D)  2
E)  1F) D) and E)
G) A) and E)

Question 3

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm, P(NO) eq = 0.10 atm, P(Cl2) eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

Accepted Answer

A)  3.7 × 10-2 atm
B)  60 atm
C)  27 atm
D)  1.7 × 10-2 atm
E)  1.8 × 10-3 atmF) B) and E)
G) A) and E)

Question 4

Calculate P (NO) eq, if P(NOCl) eq = 0.33 bar, P(Cl2) eq = 0.50 bar, and Kp = 1.9 × 10-2 bar . 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

Accepted Answer

A)  1.7 bar
B)  0.0042 bar
C)  0.30 bar
D)  0.064 bar
E)  0.087 barF) A) and C)
G) B) and E)

Question 5

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Accepted Answer

A)  The reaction will shift in the direction of products.
B)  No effect will be observed.
C)  The reaction will shift in the direction of reactants.
D)  The equilibrium constant will decrease.
E)  The equilibrium constant will increase.F) A) and D)
G) D) and E)

Question 6

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g) . N2O4(g) ⇌ 2NO2(g)  Kc = 0.21 M
[N2O4]eq = 0.039 mol L-1

Accepted Answer

A)  1.22 mol L-1
B)  9.0 × 10-2 mol L-1
C)  7.8 × 10-2 mol L-1
D)  8.2 × 10-3 mol L-1
E)  11 mol L-1F) A) and B)
G) A) and E)

Question 7

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Accepted Answer

Yes, they can have the same value. Since...

Question 8

Consider the following reaction: CH4(g) + 2H2S(g) ⇌ CS2(g) + 4H2(g) 
A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1) for the reaction.

Accepted Answer

A)  0.23 mol2 L-2
B)  0.038 mol2 L-2
C)  2.9 mol2 L-2
D)  10. mol2 L-2
E)  0.34 mol2 L-2F) A) and D)
G) B) and C)

Question 9

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H2. D2(g) + H2(g) ⇌ 2HD(g) Kp = 1.80
P(D2) eq = 1.1 × 10-3 bar P(HD) eq = 2.7 × 10-3 bar

Accepted Answer

A)  2.7 bar
B)  1.4 bar
C)  0.73 bar
D)  3.7 × 10-3 bar
E)  8.1 × 10-4 barF) D) and E)
G) C) and D)

Question 10

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) 
At 250° 0.125 mol L-1 PCl5 is added to the flask. If Kc = 1.80 mol L-1, what are the equilibrium concentrations of each gas?

Accepted Answer

A)  [PCl5] = 0.00765 mol L-1, [PCl3] = 0.117 mol L-1, and [Cl2] = 0.117 mol L-1
B)  [PCl5] = 0.0625 mol L-1, [PCl3] = 0.335 mol L-1, and [Cl2] = 0.335 mol L-1
C)  [PCl5] = 1.80 mol L-1, [PCl3] = 1.80 mol L-1, and [Cl2] = 1.80 mol L-1
D)  [PCl5] = 3.96 mol L-1, [PCl3] = 3.83 mol L-1, and [Cl2] = 3.83 mol L-1E) All of the above
F) C) and D)

Question 11

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g) . 2SO2(g) + O2(g) ⇌ 2SO3(g)  Kc = 1.7 × 108 M-1
[SO2]eq = 0.0034 mol L-1 [O2]eq = 0.0018 mol L-1

Accepted Answer

A)  1.9 mol L-1
B)  1.0 × 103 mol L-1
C)  0.53 mol L-1
D)  9.6 × 10-4 mol L-1
E)  0.73 mol L-1F) D) and E)
G) None of the above

Question 12

Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) 
A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Accepted Answer

A)  0.78 bar
B)  0.084 bar
C)  0.012 bar
D)  0.85 bar
E)  0.048 barF) A) and C)
G) C) and D)

Question 13

The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) 
If initial concentrations are [SO2] = 6.00 mol L-1, [O2] = 0.45 mol L-1, and [SO3] = 9.00 mol L-1, the system is

Accepted Answer

A)  at equilibrium.
B)  not at equilibrium and will remain in an unequilibrated state.
C)  not at equilibrium and will shift to the left to achieve an equilibrium state.
D)  not at equilibrium and will shift to the right to achieve an equilibrium state.E) A) and B)
F) All of the above

Question 14

Why aren't solids or liquids included in an equilibrium expression?

Accepted Answer

The equilibrium constant relat...

Question 15

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2NO2(g) K = 1.46
2N2O4(g) ⇌ 4NO2(g) K = ?

Accepted Answer

A)  2.13
B)  0.685
C)  3.11
D)  1.46
E)  1.13F) C) and D)
G) B) and D)

Question 16

Match the following.

-Q > K

Accepted Answer

A)  reaction will favour formation of reactants
B)  reaction has a larger amount of products than reactants
C)  reaction favours formation of more products
D)  reverse reaction is favoured
E)  reaction does not strongly favour reactants or productsF) reaction is at equilibriumG) D) and E)
H) C) and F)

Question 17

How is the reaction quotient different from an equilibrium constant for a given reaction?

Accepted Answer

The expressions for both are identical. ...

Question 18

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Accepted Answer

A)  The reaction will shift in the direction of products.
B)  No effect will be observed.
C)  The reaction will shift in the direction of reactants.
D)  The equilibrium constant will decrease.
E)  The equilibrium constant will increase.F) D) and E)
G) A) and E)

Question 19

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO2(g) + O2(g) ⇌ 2SO3(g)

Accepted Answer

A)  raising the temperature
B)  removing SO3
C)  adding O2
D)  increasing the pressure
E)  adding SO2F) All of the above
G) C) and E)

Question 20

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g) . NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) Kc = 1.58 × 10-8 M3
[NH3]eq = 2.9 × 10-3 mol L-1

Accepted Answer

A)  0.053 mol L-1
B)  4.6 × 10-11 mol L-1
C)  1.9 × 10-3 mol L-1
D)  5.4 × 10-6 mol L-1
E)  0.022 mol L-1F) B) and C)
G) B) and E)

Exam 14: Chemical Equilibrium

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g) . N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M [N2O4]eq = 0.039 mol L-1

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Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

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Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Correct AnswerverifiedYes, they can have the same value. Since...View AnswerShow Answer

Calculate P (NO) eq, if P(NOCl) eq = 0.33 bar, P(Cl2) eq = 0.50 bar, and Kp = 1.9 × 10-2 bar . 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

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Consider the following reaction: CH4(g) + 2H2S(g) ⇌ CS2(g) + 4H2(g) A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1) for the reaction.

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The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) If initial concentrations are [SO2] = 6.00 mol L-1, [O2] = 0.45 mol L-1, and [SO3] = 9.00 mol L-1, the system is

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Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Correct AnswerverifiedShow Answer

Why aren't solids or liquids included in an equilibrium expression?

Correct AnswerverifiedThe equilibrium constant relat...View AnswerShow Answer

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0.125 mol L-1 PCl5 is added to the flask. If Kc = 1.80 mol L-1, what are the equilibrium concentrations of each gas?

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H2. D2(g) + H2(g) ⇌ 2HD(g) Kp = 1.80 P(D2) eq = 1.1 × 10-3 bar P(HD) eq = 2.7 × 10-3 bar

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Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm, P(NO) eq = 0.10 atm, P(Cl2) eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

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The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g) ⇌ H2(g) + D2(g) K = 0.28 2H2(g) + 2D2(g) ⇌ 4HD(g) K = ?

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The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2NO2(g) K = 1.46 2N2O4(g) ⇌ 4NO2(g) K = ?

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The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO2(g) + O2(g) ⇌ 2SO3(g)

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g) . 2SO2(g) + O2(g) ⇌ 2SO3(g) Kc = 1.7 × 108 M-1 [SO2]eq = 0.0034 mol L-1 [O2]eq = 0.0018 mol L-1

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Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g) . NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) Kc = 1.58 × 10-8 M3 [NH3]eq = 2.9 × 10-3 mol L-1

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Match the following. -Q > K

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How is the reaction quotient different from an equilibrium constant for a given reaction?

Correct AnswerverifiedThe expressions for both are identical. ...View AnswerShow Answer

For the following reaction, what is Δn required in the conversion of Kc to Kp? 2SO2(g) + O2(g) ⇌ 2SO3(g)

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 0.039 mol L^-1

Correct Answer
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Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

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Can the K_p and K_c for a reaction ever have the same value? Why or why not?

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Yes, they can have the same value. Since...
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Calculate P (NO) _eq, if P(NOCl) _eq = 0.33 bar, P(Cl₂) _eq = 0.50 bar, and K_p = 1.9 × 10^-2 bar . 2NOCl(g) ⇌ 2NO(g) + Cl₂(g)

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Consider the following reaction: CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1) for the reaction.

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The equilibrium constant is equal to 5.00 L mol^-1 at 1300 K for the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) If initial concentrations are [SO₂] = 6.00 mol L^-1, [O₂] = 0.45 mol L^-1, and [SO₃] = 9.00 mol L^-1, the system is

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Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Correct Answer
verified

Correct Answer
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The equilibrium constant relat...
View Answer

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250° 0.125 mol L^-1 PCl₅ is added to the flask. If K_c = 1.80 mol L^-1, what are the equilibrium concentrations of each gas?

Correct Answer
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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H₂. D₂(g) + H₂(g) ⇌ 2HD(g) K_p = 1.80 P(D₂) _eq = 1.1 × 10^-3bar P(HD) _eq = 2.7 × 10^-3 bar

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Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm, P(NO) _eq = 0.10 atm, P(Cl₂) _eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl₂(g)

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The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g) ⇌ H₂(g) + D₂(g) K = 0.28 2H₂(g) + 2D₂(g) ⇌ 4HD(g) K = ?

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The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2NO₂(g) K = 1.46 2N₂O₄(g) ⇌ 4NO₂(g) K = ?

Correct Answer
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The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Correct Answer
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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₃(g) . 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) K_c = 1.7 × 10⁸M^-1 [SO₂]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

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Consider the following reaction: NO(g) + SO₃(g) ⇌ NO₂(g) + SO₂(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃. Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8M³ [NH₃]_eq = 2.9 × 10^-3 mol L^-1

Correct Answer
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Correct Answer
verified

Correct Answer
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The expressions for both are identical. ...
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For the following reaction, what is Δn required in the conversion of K_c to K_p? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

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