Deck 13: Chemical Equilibrium

Question 1

The K_a for HCN is 6.20 × 10⁻¹⁰. The concentration of CN^- in the ionization of 0.0400 M HCN in H₂O is 4.89 × 10⁻⁶ M

Answer 1

False

Question 2

Given: To maximize the reactants in the reaction above, the temperature of the reaction should be decreased.

Answer 2

False

Question 3

Given: Increasing the temperature in the reaction above shifts the equilibrium toward the reactants.

Answer 3

True

Question 4

Given: Decreasing the pressure in the reaction above shifts the equilibrium toward the reactants.

Question 5

The equilibrium equation that exists between calcium sulfate and water as reactants and calcium hydroxide and sulfuric acid as products can be represented as

Question 6

Equilibrium reactions do not stop; both the forward and reverse reaction continue to occur.

Question 7

The equilibrium concentration of H₂S(g) in the reaction below is 0.17 M.

Question 8

Given: To maximize the amount of N₂O₄ in the reaction above, the number of moles of NO₂ should be increased.

Question 9

A catalyst does not affect the extent or position of a reaction at equilibrium.

Question 10

In a chemical equilibrium reaction all the three phases of matter are included. This equation is in a state of homogeneous equilibrium.

Question 11

Given: If [C₂H₆], [O₂], [CO₂], and K_eq are 0.451 M, 0.589 M, 0.638 M, and 25.0, respectively, the equilibrium [H₂O] is 0.326 M.

Question 12

Chemical equilibrium is static rather than dynamic.

Question 13

Given: If the K_eq at 57.0°C for the reaction above is 13.6, then K_P is 0.0474.
Assume R = 0.08205

Question 14

Given: If [C₂H₆], [O₂], [CO₂], and K_eq are 0.451 M, 0.589 M, 0.638 M, and 25.0, respectively, the equilibrium [H₂O] is 0.632 M.

Question 15

The K_a for HClO₂ is 1.10 × 10⁻². The pH of 0.165 M HClO₂ in H₂O is 1.37.

Question 16

An equilibrium equation should be balanced.

Question 17

The equilibrium concentration of H₂O(g) for the chemical reaction below is 0.900 M.

Question 18

Given: The equilibrium partial pressures of [H₂O₂] and [O₂] are 1.45 atm and 1.89 atm, respectively. If K_P = 6.00 the equilibrium partial pressure of H₂O is 0.134 atm.

Question 19

For a given reaction , the equilibrium constant can be defined as .

Question 20

Given: If [HCl], [Cl₂], and K_eq are 0.586 M, 0.486 M, and 2.37, respectively, the equilibrium [H₂] is 3.35 M.

Question 21

What is the expression for for this reaction?

A)
B)
C)
D)
E)

Question 22

If the equilibrium partial pressures of [PCl₅], [PCl₃], and [Cl₂] are 0.240 atm, 0.291 atm, and 0.655 atm, respectively, determine K_P.

A) 3.14
B) 1.43
C) 1.26
D) 4.31
E) 4.13
Refer to the reaction below for 38-39.
Given:

Question 23

If [C₂H₂], [O₂], [H₂O], and [CO₂] are 0.295 M, 0.400 M, 0.500 M, and 0.686 M, respectively, determine K_eq.

A) 84.4
B) 48.4
C) 62.3
D) 42.2
E) 22.4
Refer to the reaction below for 34-35.
Given:

Question 24

What is the K_eq expression for the reaction?

A)
B)
C)
D)
E)

Question 25

What is the K_eq expression for the reaction?

A)
B)
C)
D)
E)

Question 26

What is the K_eq expression for the reaction?

A)
B)
C)
D)
E)

Question 27

What is the K_P at 37.0°C for this reaction if the K_eq is 1.20 × 10⁻²? Assume R = 0.08205

A) 4.27 * 10^{- 4}
B) 2.47 *10^{- 4}
C) 2.74 * 10^{- 4}
D) 7.42 * 10^{- 4}
E) 4.72 *10^{- 4}

Question 28

What is the K_eq expression for the reaction?

A)
B)
C)
D)
E)

Question 29

If [H₂], [Br₂], and [HBr] are 0.0350 M, 0.0600 M, and 0.0850 M, respectively, determine K_eq.

A) 6.00
B) 4.50
C) 3.44
D) 1.80
E) 404
Refer to the reaction below for 30-31.
Given:

Question 30

The equilibrium partial pressures of [H₂O₂] and [O₂] are 0.239 atm and 0.281 atm, respectively. If K_P = 5.00, determine the equilibrium partial pressure of [H₂O].

A) 2.20 atm
B) 0.220 atm
C) 0.0022 atm
D) 0.022 atm
E) 0.202 atm

Question 31

If [C₂H₆], [O₂], [CO₂], and K_eq are 0.391 M, 0.486 M, 0.400 M, and 25.0, respectively, determine the equilibrium [H₂O].

A) 0.993 M
B) 0.339 M
C) 0.393 M
D) 0.933 M
E) 0.399 M
Refer to the reaction below for 36-37.
Given:

Question 32

If the K_b for CN⁻ is 1.6 × 10⁻⁵, K_a for HCN is 6.3 × 10⁻¹⁰.

Question 33

If [OH⁻] is 2.02 × 10⁻⁷ M, [H⁺] in a solution is 4.59 × 10⁻⁸.

Question 34

If [H₂], [Cl₂], and K_eq are 0.315 M, 0.218 M, and 3.85, respectively, determine the equilibrium [HCl].

A) 0.240 M
B) 0.514 M
C) 0.0354 M
D) 0.134 M
E) 0.0530 M
Refer to the reaction below for 32-33.
Given:

Question 35

Write the equilibrium equation that exists between calcium sulfate as a reactant and calcium oxide and sulfur trioxide as products.

A)
B)
C)
D)
E)
Refer to the reaction below for 28-29.
Given:

Question 36

Write the equilibrium equation that exists between hydrogen and chlorine as reactants and hydrogen chloride as a product.

A)
B)
C)
D)
E)

Question 37

What is the K_P expression for the reaction?

A)
B)
C)
D)
E)

Question 38

If the K_sp of SrSO₄(s) is 3.8 × 10⁻⁴, the concentration of [SO₄^2-] in a saturated solution of SrSO₄(s) is 9.1 × 10⁻¹² M.

Question 39

What is the K_P at 47.0°C for this reaction if the K_eq is 2.36? Assume R = 0.08205

A) 31.2
B) 9.88
C) 0.0988
D) 62.0
E) 0.0889

Question 40

The expression for the slight solubility of Al₂(SO₄)₃(s) is .

Question 41

What is the K_eq at 7.00°C for this reaction if the K_P is 0.00123? Assume R = 0.08205

A) 19.4
B) 14.9
C) 49.1
D) 1.94
E) 1.49

Question 42

Which of the following will cause the equilibrium to shift toward the products side?

A) Removal of CO
B) Increasing the pressure
C) Addition of CO₂
D) Removal of the catalyst
E) Increasing the temperature

Question 43

Which of the following will cause the equilibrium to shift toward the products?

A) Addition of N₂
B) Addition of H₂
C) Removal of NH₃
D) Increasing the pressure
E) Increasing the temperature

Question 44

Which of the following is the right ICE chart for the reaction below?

A)
B)
C)
D)
E)

Question 45

If concentration is defined as x, formulate K_eq for the reaction given below.

A)
B)
C)
D)
E)

Question 46

What is the correct expression for the concentration of [C₂H₂I₄] in this reaction?

A)
B)
C)
D)
E)

Question 47

Determine the equilibrium concentration of HCN(g) for this reaction.

A) 3.27 M
B) 2.37 M
C) 0.372 M
D) 0.370 M
E) 0.730 M

Question 48

To maximize the amount of CO the:

A) pressure of the reaction should be reduced.
B) temperature of the reaction should be reduced.
C) number of moles of CO₂ in the reaction should be reduced.
D) amount of catalyst added should be increased.
E) number of moles of CO in the reaction should be increased.

Question 49

If concentration is defined as x, formulate K_eq for the reaction given below.

A)
B)
C)
D)
E)

Question 50

Determine the equilibrium concentration of H₂(g) for this reaction.

A) 0.039 M
B) 0.0039 M
C) 0.39 M
D) 0.093 M
E) 0.0093 M

Question 51

Which of the following will cause the equilibrium to shift toward the reactants side?

A) Addition of CO
B) Removal of CO₂
C) Removal of the catalyst
D) Increasing the temperature
E) Increasing the pressure

Question 52

To maximize the amount of N₂ the:

A) pressure of the reaction should be reduced.
B) temperature of the reaction should be decreased.
C) amount of catalyst added should be increased.
D) number of moles of N₂ in the reaction should be increased.
E) number of moles of NH₃ in the reaction should be reduced.
Refer to the reaction below for 50-53.
Given:

Question 53

To maximize the amount of NH₃ the:

A) pressure of the reaction should be reduced.
B) temperature of the reaction should be reduced.
C) number of moles of H₂ in the reaction should be reduced.
D) number of moles of N₂ in the reaction should be reduced.
E) number of moles of NH₃ in the reaction should be increased.

Question 54

Determine the equilibrium concentration of CO(g) for this reaction.

A) 0.836 M
B) 0.683 M
C) 0.386 M
D) 0.863 M
E) 0.368 M

Question 55

To maximize the amount of CO₂ the:

A) pressure of the reaction should be reduced.
B) temperature of the reaction should be increased.
C) number of moles of CO₂ in the reaction should be increased.
D) amount of catalyst added should be reduced.
E) number of moles of CO in the reaction should be increased.

Question 56

Determine the equilibrium concentration of N₂O₃(g) for this reaction.

A) 1.76 M
B) 1.23 M
C) 5.61 M
D) 1.65 M
E) 6.51 M

Question 57

What is the correct K_eq expression for this reaction?

A)
B)
C)
D)
E)

Question 58

Determine the equilibrium concentration of Cl₂(g) for this reaction.

A) 0.729 M
B) 9.27 M
C) 2.97 M
D) 9.72 M
E) 0.297 M

Question 59

What is the correct K_P expression for this reaction?

A)
B)
C)
D)
E)
Refer to the reaction below for 46-49.
Given:

Question 60

Which of the following will cause the equilibrium to shift toward the reactants?

A) Removal of N₂
B) Removal of H₂
C) Removal of NH₃
D) Reducing the pressure
E) Increasing the temperature

Question 61

What is the concentration of [Ag⁺] in a saturated solution of AgI? The K_sp of AgI is 9.50 × 10⁻¹⁷.

A) 9.75 × 10⁻⁹ M
B) 2.92 × 10⁻¹⁰ M
C) 6.20 × 10⁻¹⁰ M
D) 2.60 × 10⁻⁹ M
E) 2.29 × 10⁻⁹ M

Question 62

Which of the following is the equilibrium equation for HF acting as a weak acid?

A)
B)
C)
D)
E)

Question 63

What is the pOH of a 0.500 M solution of HClO₂? The K_a of HClO₂ is 1.10 × 10⁻².

A) 1.13
B) 12.9
C) 3.11
D) 11.3
E) 31.1

Question 64

Describe chemical equilibrium as a dynamic process.

Question 65

What is the effect of temperature changes on an equilibrium?

Question 66

Explain the law of mass action and equilibrium constant.

Question 67

How does the addition or removal of a product or a reactant affect the equilibrium of a reaction?

Question 68

What is the concentration of [Ag⁺] in a saturated solution of Ag₂SO₄? The K_sp of Ag₂SO₄ is 1.50 × 10⁻⁵.

A) 0.0155 M
B) 0.0310 M
C) 0.0465 M
D) 0.0620 M
E) 0.0775 M

Question 69

What is the concentration of [PO₄^3-] in a saturated solution of Ca₃(PO₄)₂? The K_sp of Ca₃(PO₄)₂ is 2.1 × 10⁻³³.

A) 3.28 × 10⁻⁶ M
B) 1.64 × 10⁻⁶ M
C) 2.82 × 10⁻⁷ M
D) 2.28 × 10⁻⁷ M
E) 8.22 × 10⁻⁷ M

Question 70

How do we define the equilibrium constant in terms of partial pressures?

Question 71

What is the K_sp expression for Mg₃(PO₄)₂?

A)
B)
C)
D)
E)

Question 72

How does an equilibrium react to a change in pressure?

Question 73

Define Le Chatelier's principle. If a reaction is exothermic, if the temperature is increased, what which way will the reaction shift?

Question 74

Explain the relationship between K_eq and K_P.

Question 75

What is the value of K_b for CN^-, which can accept a proton and act as a base? The K_a for HCN is 6.20 × 10⁻¹⁰.

A) 6.20 × 10⁻¹⁰
B) 2.60 × 10⁻⁵
C) 1.16 × 10⁻⁵
D) 6.11 × 10⁻⁵
E) 1.61 × 10⁻⁵

Question 76

Explain heterogeneous equilibrium with an example. What is the rule for heterogeneous equilibria?

Question 77

Define chemical equilibrium with an example.

Question 78

What is the pH of a 0.600 M solution of H₂PO₄⁻? The K_a of H₂PO₄⁻ is 6.2 × 10⁻⁸.

A) 3.71
B) 10.3
C) 3.10
D) 30.1
E) 17.7

Question 79

Which of the following is the K_a expression for HSO₄^- acting as a weak acid?

A)
B)
C)
D)
E)

Question 80

Explain the importance of the equilibrium constant.