Deck 14: Chemical Equilibrium

Question 1

What is △n for the following equation in relating K_c to K_p?
N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A)4
B)-4
C)-2
D)2
E)1

Answer 1

-2

Question 2

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

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

Answer 2

8.1

Question 3

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
2 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

Answer 3

2.6 × 10^-5

Question 4

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

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

Question 5

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 6

Express the equilibrium constant for the following reaction.
N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

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

Question 7

In which of the following reactions will K_c = K_p?

A)H₂(g)+ I₂(g)⇌ 2 HI(g)
B)CH₄(g)+ H₂O(g)⇌ CO(g)+ 3 H₂(g)
C)N₂O₄(g)⇌ 2NO₂(g)
D)CO(g)+ 2 H₂(g)⇌ CH₃OH(g)
E)N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

Question 8

Express the equilibrium constant for the following reaction.
H₂(g)+ Br₂(g)⇌ 2 HBr(g)

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

Question 9

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)0.63

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

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
N₂O₄(g)⇌ 2 NO₂(g)K_c = 1.46
3 N₂O₄(g)⇌ 6 NO₂(g)K_c = ?

A)2.13
B)0.685
C)3.11
D)1.46
E)1.13

Question 12

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 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.
2 HD(g)⇌ H₂(g)+ D₂(g)K_c = 0.28
2 H₂(g)+ 2 D₂(g)⇌ 4 HD(g)K_c = ?

A)7.8 × 10^-2
B)3.6
C)0.53
D)13
E)1.9

Question 15

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

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

Question 16

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 17

What is △n for the following equation in relating K_c to K_p?
2 NH₃(g)⇌ N₂(g)+ 3 H₂(g)

A)4
B)-4
C)-2
D)2
E)1

Question 18

What is △n for the following equation in relating K_c to K_p?
H₂(g)+ Br₂(g)⇌ 2 HBr(g)

A)0
B)-1
C)-2
D)2
E)1

Question 19

Express the equilibrium constant for the following reaction.
2 P(g)+ 3 Cl₂(g)⇌ 2 PCl₃(g)

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

Question 20

What is △n for the following equation in relating K_c to K_p?
2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

A)3
B)-1
C)-2
D)2
E)1

Question 21

Which of the following statements are true?

A)Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
B)The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction.
C)A reaction quotient (Q)larger than the equilibrium constant (K)means that the reaction will favor the production of more products.
D)Dynamic equilibrium indicates that the amount of reactants and products are equal.
E)All of the above are true.

Question 22

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 23

For which reaction will K_p = K_c?

A)S(s)+ O₂(g)⇌ SO₂(g)
B)2 HgO(s)⇌ Hg(l)+ O₂(g)
C)CaCO₃(s)⇌ CaO(s)+ CO₂(g)
D)H₂CO₃(s)⇌ H₂O(l)+ CO₂(g)
E)2 H₂O(l)⇌ 2 H₂(g)+ O₂(g)

Question 24

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 25

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 26

The reaction below has a K_c value of 61.What is the value of K_p for this reaction at 500 K?
N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A)15
B)61
C)28
D)3.6 × 10^-2
E)1.9 × 10^-2

Question 27

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 28

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

Question 29

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 500 K?
2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

A)4.2 × 10^-11
B)1.0 × 10¹²
C)2.4 × 10^-12
D)4.1 × 10¹³
E)2.4 × 10¹⁰

Question 30

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)2.9 × 10³¹
C)1.2 × 10¹⁷
D)1.4 × 10^-19
E)3.5 × 10^-32

Question 31

Express the equilibrium constant for the following reaction.
P₄(s)+ 5 O₂(g)⇌ P₄O₁₀(s)

A)K =
B)K =
C)K = [O₂]^-5
D)K = [O₂]⁵
E)K =

Question 32

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

Question 33

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 34

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 M,[PCl₃]_eq = 0.23 M,[Cl₂]_eq = 4.4 M.
PCl₅(g)⇌ PCl₃(g)+ Cl₂(g)

A)1.8
B)0.93
C)0.55
D)1.1
E)0.76

Question 35

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M.
H₂(g)+ I₂(g)⇌ 2 HI(g)

A)2.1 × 10^-2
B)29
C)47
D)3.4 × 10^-2
E)8.7 × 10^-2

Question 36

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K?
N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A)2.4 × 10^-2
B)4.4 × 10⁴
C)41
D)2.3 × 10^-5
E)1.9 × 10⁴

Question 37

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 38

Express the equilibrium constant for the following reaction.
2 Na(s)+ 2 H₂O(l)⇌ 2 NaOH(aq)+ H₂(g)

A)K =
B)K = [H₂][NaOH]^-2
C)K =
D)K = [H₂][NaOH]²
E)K =

Question 39

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.
2 NOCl(g)? 2 NO(g)+ Cl₂₍g)

A)3.7 × 10^-2
B)60.
C)27
D)1.7 × 10^-2
E)1.8 × 10^-3

Question 40

Express the equilibrium constant for the following reaction.
KClO₃(s)⇌ KClO(s)+ O₂(g)

A)K =
B)K = [O₂]^-1
C)K =
D)K =
E)K = [O₂]

Question 41

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 42

Consider the following reaction and its equilibrium constant:
I₂(g)⇌ 2I(g)K_p = 0.209
A reaction mixture contains 0.89 atm I₂ and 1.77 atm I.Which of the following statements is true concerning this system?

A)The reaction will shift in the direction of reactants.
B)The reaction quotient will increase.
C)The reaction will shift in the direction of products.
D)The equilibrium constant will decrease.
E)The system is at equilibrium.

Question 43

Consider the following reaction and its equilibrium constant:
SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)K_c = 0.33
A reaction mixture contains 0.39 M SO₂,0.14 M NO₂,0.11 M SO₃ and 0.14 M NO.Which of the following statements is true concerning this system?

A)The reaction will shift in the direction of reactants.
B)The equilibrium constant will decrease.
C)The reaction will shift in the direction of products.
D)The reaction quotient will decrease.
E)The system is at equilibrium.

Question 44

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 45

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 46

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 47

Consider the following reaction:
COCl₂(g)⇌ CO(g)+ Cl₂(g0
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 48

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 49

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

A)0.053 M
B)4.6 × 10^-11 M
C)1.9 × 10^-3 M
D)5.4 × 10^-6 M
E)0.022 M

Question 50

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

A)1.22 M
B)9.0 × 10^-2 M
C)7.8 × 10^-2 M
D)8.2 × 10^-3 M
E)11 M

Question 51

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 52

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

A)No effect will be observed since C 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 53

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 54

Consider the following reaction and its equilibrium constant:
4 CuO(s)+ CH₄(g)⇌ CO₂(g)+ 4 Cu(s)+ 2 H₂O(g)K_c = 1.10
A reaction mixture contains 0.22 M CH₄,0.67 M CO₂ and 1.3 M H₂O.Which of the following statements is true concerning this system?

A)The reaction will shift in the direction of products.
B)The equilibrium constant will increase.
C)The reaction quotient will increase.
D)The reaction will shift in the direction of reactants.
E)The system is at equilibrium.

Question 55

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 56

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 57

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 58

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 59

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 60

Consider the following reaction and its equilibrium constant:
I₂(g)+ Br₂(g)⇌ 2 IBr(g)K_c = 1.1 × 10²
A reaction mixture contains 0.41 M I₂,0.27 M Br₂ and 3.5 M IBr.Which of the following statements is true concerning this system?

A)The reaction will shift in the direction of products.
B)The reaction will shift in the direction of reactants.
C)The reaction quotient will decrease.
D)The equilibrium constant will increase.
E)The system is at equilibrium.

Question 61

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 62

Why is an equilibrium constant unitless?

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 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 65

Consider the following reaction at equilibrium.What effect will adding 1 atm of Ar to 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 66

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 67

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 68

Consider the following reaction at equilibrium.What effect will adding water 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 69

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 70

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

Question 71

Match the following.
Q < K

A)Reaction will favor formation of reactants.
B)Reaction does not strongly favor reactants or products.
C)Reaction favors formation of more products.
D)Reaction has a larger amount of products than reactants.
E)Reaction is at equilibrium.

Question 72

Match the following.
Q = K

A)Reaction will favor formation of reactants.
B)Reaction does not strongly favor reactants or products.
C)Reaction favors formation of more products.
D)Reaction has a larger amount of products than reactants.
E)Reaction is at equilibrium.

Question 73

Match the following.
K ≈ 1

A)Reaction will favor formation of reactants.
B)Reaction does not strongly favor reactants or products.
C)Reaction favors formation of more products.
D)Reaction has a larger amount of products than reactants.
E)Reaction is at equilibrium.

Question 74

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 75

Match the following.
Q >> 1

A)Reaction will favor formation of reactants.
B)Reaction does not strongly favor reactants or products.
C)Reaction favors formation of more products.
D)Reaction has a larger amount of products than reactants.
E)Reaction is at equilibrium.

Question 76

Match the following.
K << 1

A)Reaction will favor formation of reactants.
B)Reaction does not strongly favor reactants or products.
C)Reaction favors formation of more products.
D)Reaction has a larger amount of products than reactants.
E)Reaction is at equilibrium.

Question 77

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

Question 78

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 79

Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

Question 80

Consider the following reaction at equilibrium.What effect will adding a catalyst 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.