Deck 15: Chemical Equilibrium

Question 1

The reaction below has a K_p value of 3.3 × 10^-5.What is the value of K_c for this reaction at 700 K? 2 SO₃(g)⇌ 2 SO₂(g)+ O₂(g)

A) 5.7 × 10^-7
B) 1.7 × 10⁶
C) 3.3 × 10^-5
D) 3.0 × 10⁴
E) 1.9 × 10^-3

Answer 1

5.7 × 10^-7

Question 2

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ 2 HBr(g)K_c = 3.8 × 10⁴
4 HBr(g)⇌ 2 H₂(g)+ 2 Br₂(g)K_c = ?

A) 1.9 × 10⁴
B) 5.1 × 10^-3
C) 2.6 × 10^-5
D) 6.9 × 10^-10
E) 1.6 × 10³

Answer 2

6.9 × 10^-10

Question 3

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 M,[H₂]_eq = 1.1 M,[NH₃]_eq = 0.47 M. N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A) 3.5
B) 0.28
C) 9.1
D) 0.11
E) 0.78

Answer 3

0.11

Question 4

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)K_c = 1.7 × 10⁶
SO₃(g)⇌ 1/2 O₂(g)+ SO₂(g)K_c = ?

A) 3.4 × 10²
B) 8.5
C) 1.3 × 10³
D) 1.2 × 10^-6
E) 7.7 × 10^-4

Question 5

Express the equilibrium constant for the following reaction. Pb(NO₃)₂(aq)+ 2 NaI(aq)⇌ PbI₂(s)+ 2 NaNO₃(aq)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 6

Which of the following statements is FALSE?

A) When K >> 1, the forward reaction is favored and essentially goes to completion.
B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
C) When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.
D) K >> 1 implies that the reaction is very fast at producing products.
E) None of the above.

Question 7

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. 2 A(g)+ B(g)⇌ A₂B(g)Kc = ?
A₂B(g)+ B(g)⇌ A₂B₂(g)K_c = 16.4
2 A(g)+ 2 B(g)⇌ A₂B₂(g)K_c = 28.2

A) 11.8
B) 0.00216
C) 0.582
D) 462
E) 1.72

Question 8

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g)+ B(g)⇌ AB(g)Kc = 0.24
AB(g)+ A(g)⇌ A₂B(g)K_c = 3.8
2 A(g)+ B(g)⇌ A₂B(g)K_c = ?

A) 4.0
B) 0.91
C) 3.6
D) 16
E) 0.063

Question 9

Express the equilibrium constant for the following reaction. 4 Al(s)+ 3 O₂(g)⇌ 2 Al₂O₃(s)

A) K =
B) K =
C) K =
D) K = [O₂]³
E) K = [3O₂]³

Question 10

In which of the following reactions will K_c = K_p?

A) 4 NH₃(g) + 3 O₂(g) ⇌ 2 N₂(g) + 6 H₂O(g)
B) SO₃(g) + NO(g) ⇌ SO₂(g) + NO₂(g)
C) 2 N₂(g) + O₂(g) ⇌ 2 N₂O(g)
D) 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)
E) None of the above reactions have K_c = K_p.

Question 11

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 3.6 M,[O₂]_eq = 4.1 M,[N₂O]_eq = 3.3 × 10^-18 M. 2 N₂(g)+ O₂(g)⇌ 2 N₂O(g)

A) 2.2 × 10^-19
B) 4.5 × 10¹⁸
C) 2.0 × 10^-37
D) 5.0 × 10³⁶
E) 4.9 × 10^-17

Question 12

Give the direction of the reaction,if K >> 1.

A) The forward reaction is favored.
B) The reverse reaction is favored.
C) Neither direction is favored.
D) If the temperature is raised, then the forward reaction is favored.
E) If the temperature is raised, then the reverse reaction is favored.

Question 13

Give the direction of the reaction,if K ≈ 1.

A) The forward reaction is favored.
B) The reverse reaction is favored.
C) Neither direction is favored.
D) If the temperature is raised, then the forward reaction is favored.
E) If the temperature is raised, then the reverse reaction is favored.

Question 14

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ HBr(g)K_c = 3.8 × 10⁴
HBr(g)⇌ H₂(g)+ Br₂(g)K_c = ?

A) 1.9 × 10⁴
B) 5.3 × 10^-5
C) 2.6 × 10^-5
D) 6.4 × 10^-4
E) 1.6 × 10³

Question 15

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [P₄O₁₀]_eq = 2.000 moles,[P₄]_eq = 3.000 moles,[O₂]_eq = 4.000 M P₄O₁₀(s)⇌ P₄(s)+ 5 O₂(g)

A) 20.00
B) 4.000
C) 1.320
D) 1536
E) 1024

Question 16

Express the equilibrium constant for the following reaction. CH₄(g)+ 2 O₂(g)⇔ CO₂(g)+ 2 H₂O(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 17

Hemoglobin carries ________ in the blood.

A) nitrogen
B) hydrogen
C) oxygen
D) carbon
E) sodium

Question 18

Define dynamic equilibrium.

A) no reactants react
B) no products are formed
C) the rate of the forward reaction is faster than the rate of the reverse reaction
D) the rate of the reverse reaction is faster than the rate of the forward reaction
E) the rate of the forward reaction equals the rate of the reverse reaction

Question 19

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g)+ 2 B(g)⇌ AB₂(g)Kc = 59
AB₂(g)+ B(g)⇌ AB₃(g)K_c = ?
A(g)+ 3 B(g)⇌ AB₃(g)K_c = 478

A) 3.5 × 10^-5
B) 2.8 × 10⁴
C) 8.1
D) 0.12
E) 89

Question 20

Give the direction of the reaction,if K << 1.

A) The forward reaction is favored.
B) The reverse reaction is favored.
C) Neither direction is favored.
D) If the temperature is raised, then the forward reaction is favored.
E) If the temperature is raised, then the reverse reaction is favored.

Question 21

In a reaction mixture containing reactants and products,each at a concentration of 1M,what is the value of Q?

A) -1
B) 1
C) ∞
D) 0
E) It cannot be determined without concentrations.

Question 22

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g). C₂H₄(g)+ H₂O(g)⇌ C₂H₅OH(g)K_c = 9.0 × 10³
[C₂H₄]_eq = 0.015 M [C₂H₅OH]_eq = 1.69 M

A) 9.9 × 10^-7 M
B) 80. M
C) 1.0 M
D) 1.68 M
E) 0.013 M

Question 23

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

A) 2.8 × 10¹³ M
B) 1.88 M
C) 6.1 × 10^-6 M
D) 1.0 × 10³ M
E) 1.4 M

Question 24

Consider the following reaction: COCl₂(g)⇌ CO(g)+ Cl₂(g)
A reaction mixture initially contains 1.6 M COCl₂.Determine the equilibrium concentration of CO if K_c for the reaction at this temperature is 8.33 × 10^-4.Calculate this based on the assumption that the answer is negligible compared to 1.6.

A) 4.2 × 10^-4 M
B) 1.5 × 10^-3 M
C) 3.7 × 10^-2 M
D) 2.1 × 10^-2 M
E) 1.3 × 10^-3 M

Question 25

In a reaction mixture containing only products,what is the value of Q?

A) -1
B) 1
C) ∞
D) 0
E) It cannot be determined without concentrations.

Question 26

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO. CO(g)+ 2 H₂(g)⇌ CH₃OH(l)K_p = 2.25 × 10⁴
P(H₂)_eq = 0.52 atm

A) 8.3 × 10⁴ atm
B) 1.2 × 10^-5 atm
C) 6.25 × 10^-3 atm
D) 8.5 × 10^-5 atm
E) 1.6 × 10^-4 atm

Question 27

In a reaction mixture containing only reactants,what is the value of Q?

A) -1
B) 1
C) ∞
D) 0
E) It cannot be determined without concentrations.

Question 28

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

A) 0.23
B) 0.038
C) 2.9
D) 10.
E) 0.34

Question 29

Which of the following statements is TRUE?

A) Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at any point in the reaction.
B) Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at any point in the reaction.
C) Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at equilibrium.
D) Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at equilibrium.
E) Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, at the point both are equal.

Question 30

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

A) 2.7 atm
B) 1.4 atm
C) 0.73 atm
D) 3.7 × 10^-3 atm
E) 8.1 × 10^-4 atm

Question 31

Which of the following statements is TRUE?

A) If Q < K, it means the forward reaction will proceed to form more products.
B) If Q > K, it means the forward reaction will proceed to form more products.
C) If Q = K, it means the reaction is not at equilibrium.
D) All of the above are true.
E) None of the above is true.

Question 32

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

A) 1.9 M
B) 1.0 × 10³ M
C) 0.53 M
D) 9.6 × 10^-4 M
E) 0.73 M

Question 33

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(CO)_eq = 6.8 × 10^-11 atm,P(O₂)_eq = 1.3 × 10^-3 atm,P(CO₂)_eq = 0.041 atm. 2 CO(g)+ O₂(g)⇌ 2 CO₂(g)

A) 3.6 × 10^-21
B) 2.8 × 10²⁰
C) 4.6 × 10¹¹
D) 2.2 × 10^-12
E) 3.6 × 10^-15

Question 34

Which of the following statements is TRUE?

A) If Q < K, it means the reverse reaction will proceed to form more reactants.
B) If Q > K, it means the forward reaction will proceed to form more products.
C) If Q = K, it means the reaction is at equilibrium.
D) All of the above are true.
E) None of the above are true.

Question 35

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 M,[HI]_eq = 5.6 × 10^-16 M,[Cl₂]_eq = 0.0019 M. 2 HCl(g)+ I₂(s)⇌ 2 HI(g)+ Cl₂(g)

A) 8.2 × 10^-18
B) 2.8 × 10³¹
C) 1.2 × 10¹⁷
D) 1.4 × 10^-19
E) 3.5 × 10^-32

Question 36

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 M,[NH₃]_eq = 0.5 M,and K_c = 2. N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A) 0.016 M
B) 0.031 M
C) 0.062 M
D) 0.40 M
E) 62.5 M

Question 37

Consider the following reaction: Xe(g)+ 2 F₂(g)⇌ XeF₄(g)
A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F₂.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (K_p)for the reaction.

A) 25
B) 0.12
C) 0.99
D) 8.3
E) 0.040

Question 38

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 M,[HI]_eq = 5.6 × 10^-16 M,[Cl₂]_eq = 0.0019 M. 2 HI(g)+ Cl₂(g)⇌ 2 HCl(g)+ I₂(s)

A) 8.2 × 10^-18
B) 2.8 × 10³¹
C) 1.2 × 10¹⁷
D) 1.4 × 10^-19
E) 3.5 × 10^-32

Question 39

Which of the following statements is TRUE?

A) If Q < K, it means the reverse reaction will proceed to form more reactants.
B) If Q > K, it means the reverse reaction will proceed to form more reactants.
C) If Q = K, it means the reaction is not at equilibrium.
D) All of the above are true.
E) None of the above are true.

Question 40

Calculate P [NO]_eq,if P [NOCl]_eq = 0.33 atm,P [Cl₂]_eq = 0.50 atm,and K_p = 1.9 × 10^-2. 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g)

A) 1.7 atm
B) 0.0042 atm
C) 0.30 atm
D) 0.064 atm
E) 0.087 atm

Question 41

Consider the following reaction at equilibrium.What will happen if O₂ is added to the reaction? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 42

Define Le Chatelier's Principle.

A) When a chemical system at equilibrium is disturbed, the system shifts in a direction that maximizes the disturbance.
B) A system will always change if the pressure changes.
C) When a chemical system at equilibrium is disturbed, the system shifts in a direction that equals the disturbance.
D) When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance.
E) A system will always change if the volume changes.

Question 43

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

A) raising the temperature
B) adding SO₃
C) removing O₂
D) all of the above
E) none of the above

Question 44

Consider the following reaction at equilibrium.What effect will adding CO₂ have on the system? CO₂(g)+ C(graphite)⇌ 2 CO(g)

A) No effect will be observed since CO₂ is not included in the equilibrium expression.
B) The equilibrium constant will decrease.
C) The reaction will shift to the left in the direction of reactants.
D) The equilibrium constant will increase.
E) The reaction will shift to the right in the direction of products.

Question 45

Consider the following reaction: CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)
A reaction mixture initially contains 2.9 M O₂.Determine the equilibrium concentration of O₂ if K_c for the reaction at this temperature is 1.5.

A) 1.9 M
B) 1.7 M
C) 2.2 M
D) 1.2 M
E) 0.59 M

Question 46

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

A) raising the temperature
B) decrease pressure
C) increase volume
D) all of the above
E) none of the above

Question 47

Consider the following reaction at equilibrium.What will happen if Fe₂O₃ is added to the reaction? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 48

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

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

Question 49

Consider the following reaction at equilibrium.What effect will removing NO₂ have on the system? SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)

A) The reaction will shift in the direction of products.
B) The reaction will shift to decrease the pressure.
C) No change will occur since SO₃ is not included in the equilibrium expression.
D) The reaction will shift in the direction of reactants.
E) The equilibrium constant will decrease.

Question 50

Consider the following reaction at equilibrium.What will happen if SO₂ is added to the reaction? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 51

Consider the following reaction at equilibrium.What effect will adding more SO₃ have on the system? SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)

A) The reaction will shift in the direction of products.
B) The reaction will shift to decrease the pressure.
C) No change will occur since SO₃ is not included in the equilibrium expression.
D) The reaction will shift in the direction of reactants.
E) The equilibrium constant will decrease.

Question 52

Consider the following reaction: 2 H₂O(g)+ 2 SO₂(g)⇌ 2 H₂S(g)+ 3 O₂(g)
A reaction mixture initially contains 2.8 M H₂O and 2.6 M SO₂.Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6.

A) 0.045 M
B) 0.058 M
C) 0.028 M
D) 3.1 × 10^-3 M
E) 0.12 M

Question 53

Consider the following reaction: CO₂(g)+ C(graphite)⇌ 2 CO(g)
A reaction mixture initially contains 0.56 atm CO₂ and 0.32 atm CO.Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25.

A) 0.83 atm
B) 0.31 atm
C) 0.26 atm
D) 0.58 atm
E) 0.42 atm

Question 54

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

A) The reaction will shift to the left.
B) No change will be observed.
C) The equilibrium constant will decrease.
D) The equilibrium constant will increase.
E) The reaction will shift in the direction of products.

Question 55

Consider the following reaction at equilibrium.What will happen if FeS₂ is added to the reaction? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 56

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

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

Question 57

Consider the following reaction at equilibrium.What will happen if the volume increased? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 58

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

A) The reaction will shift to the left.
B) No change will be observed.
C) The equilibrium constant will decrease.
D) The equilibrium constant will increase.
E) The reaction will shift in the direction of products.

Question 59

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

A) 0.78 atm
B) 0.084 atm
C) 0.012 atm
D) 0.85 atm
E) 0.048 atm

Question 60

Consider the following reaction at equilibrium.What will happen if the pressure increased? 4 FeS₂(s)+ 11 O₂(g)⇌ 2 Fe₂O₃(s)+ 8 SO₂(g)

A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.

Question 61

Express the equilibrium constant for the following reaction. 4 CH₃Cl(g)+ 2 Cl₂(g)⇔ 4 CH₂Cl₂(g)+ 2 H₂(g)

A) K =
B) K =

C) K =

D) K =
E) K =

Question 62

Express the equilibrium constant for the following reaction. 10 N₂(g)+ 30 H₂(g)⇔ 20 NH₃(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 63

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)

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

Question 64

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

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

Question 65

Express the equilibrium constant for the following reaction. 10 PCl₅(g)⇌ 10 PCl₃(g)+ 10 Cl₂(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 66

Express the equilibrium constant for the following reaction. 12 NH₃(g)⇔ 6 N₂(g)+ 18 H₂(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 67

Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO₂(g)+ 2 H₂O(l)⇌ CH₄(g)+ 2 O₂(g)ΔH° = +890 kJ

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

Question 68

Express the reverse equilibrium constant for the following reaction. 4 CH₃Cl(g)+ 2 Cl₂(g)⇔ 4 CH₂Cl₂(g)+ 2 H₂(g)

A) K =
B) K =

C) K =

D) K =
E) K =

Question 69

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system? C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

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

Question 70

Consider the following reaction at equilibrium.What effect will reducing the pressure of the reaction mixture have on the system? Xe(g)+ 2 F₂(g)⇌ XeF₄(g)

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

Question 71

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)

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

Question 72

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2 F₂(g)⇌ XeF₄(g)

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

Question 73

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? Fe₃O₄(s)+ CO(g)⇌ 3 FeO(s)+ CO₂(g)ΔH°= +35.9 kJ

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

Question 74

Express the equilibrium constant for the following reaction. 20 CH₃Br(g)+ 10 Br₂(g)⇔ 20 CH₂Br₂(g)+ 10 H₂(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 75

Consider the following reaction at equilibrium.What effect will reducing the volume have on the system? C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

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

Question 76

Express the reverse equilibrium constant for the following reaction. 8 H₂(g)+ 8 Br₂(g)⇌ 16 HBr(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 77

Express the equilibrium constant for the following reaction. 14 P(g)+ 21 Cl₂(g)⇌ 14 PCl₃(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 78

Express the reverse equilibrium constant for the following reaction. 4 P(g)+ 6 Cl₂(g)⇌ 4 PCl₃(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 79

Express the equilibrium constant for the following reaction. 8 H₂(g)+ 8 Br₂(g)⇌ 16 HBr(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 80

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 HD(g)⇌ H₂(g)+ D₂(g)K_c = 0.28
5 H₂(g)+ 5 D₂(g)⇌ 10 HD(g)K_c = ?

A) 0.0017
B) 1.3
C) 1.34
D) 581
E) 0.76