Question 1

For which of the following values of an equilibrium constant, Keq, would you expect the equilibrium to lie farthest to the right?

Accepted Answer

A)  0.491, at 20 °C 
B)  1.04, at 20 °C 
C)  10.6, at 20 °C 
D)  1.46 × 10-4 , at 20 °C 
A)  0.491, at 20 °C 
B)  1.04, at 20 °C 
C)  10.6, at 20 °C 
D)  1.46 × 10-4 , at 20 °C

Question 2

If the solubility of copper(II) sulfate is 4.9 × 10-3 M, the solubility product is ________.

Accepted Answer

A)  2.4 × 10-5 
B)  9.6 × 10-5 
C)  1.2 × 10-2 
D)  8.7 × 10-8 
A)  2.4 × 10-5 
B)  9.6 × 10-5 
C)  1.2 × 10-2 
D)  8.7 × 10-8

Question 3

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-L? (g) + H? (g)   2 HI (g)

Accepted Answer

A) left (?) 
B) right (?) 
A) left (?) 
B) right (?)

Question 4

For the following reaction, the equilibrium constant, Keq, is equal to 53.3. What is the concentration of I₂ at equilibrium, if the concentrations of HI and H2  are 0.212 M and 1.576 M, respectively? H₂ + I₂   2HI

Accepted Answer

A)  1.576 M 
B)  0.000535 M 
C)  0.212 M 
D)  0.314 M 
A)  1.576 M 
B)  0.000535 M 
C)  0.212 M 
D)  0.314 M

Question 5

For the following exothermic reaction:
CO +       OH
predict the direction of the reaction if:
a) temperature is decreased with the concentrations remaining the same.
b) a catalyst is added with the concentrations AND temperature remaining the same.
c) the concentration of   is halved.

Accepted Answer

a) a shift to the ri

Question 6

Decreasing the volume will ________. 2SO₃ (g) + 2CL₂ (g)   2SO₂CL₂ (g) + O₂ (g)

Accepted Answer

A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown 
A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown

Question 7

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value.
-N? (g)+ 2 H? (g)   N?H? (g)
[H?] = 0.20 M, [N?] = 0.10 M, [N?H?] = 0.10 M

Accepted Answer

A) 25 
B) 12.3 
C) 5.0 
A) 25 
B) 12.3 
C) 5.0

Question 8

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-2356.3

Accepted Answer

A) Equilibrium lies to the right/ products favored 
B) Equilibrium lies to the left/reactants favored 
A) Equilibrium lies to the right/ products favored 
B) Equilibrium lies to the left/reactants favored

Question 9

If the value of the equilibrium constant for the reverse reaction is 2.5 × 10-6, the value of the equilibrium constant for the forward reaction is ________.

Accepted Answer

A)  -2.5 × 10-6 
B)  4.0 × 105 
C)  2.5 × 106 
D)  4.0 × 107 
A)  -2.5 × 10-6 
B)  4.0 × 105 
C)  2.5 × 106 
D)  4.0 × 107

Question 10

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCl3] = 0.45 M and [PCl5] = 0.73 M. Based on the calculated value of the equilibrium constant, the reaction is ________. CL₂ (g) + PCL₃ (g)   PCl5 (g)

Accepted Answer

A)  favorable 
B)  unfavorable 
C)  temperature dependent 
D)  temperature independent 
A)  favorable 
B)  unfavorable 
C)  temperature dependent 
D)  temperature independent

Question 11

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-4.23

Accepted Answer

A) Equilibrium lies to the right/ products favored 
B) Equilibrium lies to the left/reactants favored 
A) Equilibrium lies to the right/ products favored 
B) Equilibrium lies to the left/reactants favored

Question 12

Reducing the pressure will shift the equilibrium to the left.
N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Accepted Answer

A) True 
 B)False

Question 13

Increasing the pressure will ________. 2 HCl (g)   CL₂ (g) + H₂ (g)

Accepted Answer

A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown 
A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown

Question 14

If oxygen is removed this will ________. CH₄ (g) + 2O₂ (g)   CO₂ (g) + 2H₂O (g)

Accepted Answer

A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown 
A)  shift the reaction to the right 
B)  shift the reaction to the left 
C)  have no effect 
D)  cannot be determined, since the temperature is unknown

Question 15

For the following endothermic reaction:
C (s) +   (g)   2CO (g)
predict the direction of the reaction if:
a) CO concentration is increased with the temperature remaining constant.
b) some carbon (C) is removed with the temperature remaining constant)
c) the temperature is increased with the concentrations unchanged.

Accepted Answer

a) shift l

Question 16

For the following exothermic reaction, what condition will increase the yield of product? C₂H₂ (g) + H₂O (g)   CH₃CHO (g)

Accepted Answer

A)  high temperature, high pressure 
B)  high temperature, low pressure 
C)  low temperature, high pressure 
D)  low temperature, low pressure 
A)  high temperature, high pressure 
B)  high temperature, low pressure 
C)  low temperature, high pressure 
D)  low temperature, low pressure

Question 17

The equilibrium concentrations for the reaction at 673 K are [H₂] = 0.63 M, [N₂] = 0.45 M, and [NH₃] = 0.24 M. The value of Keq is ________. N₂ (g) + 3H₂ (g)   2NH₃ (g)

Accepted Answer

A)  0.85 
B)  1.18 
C)  0.51 
D)  1.96 
A)  0.85 
B)  1.18 
C)  0.51 
D)  1.96

Question 18

Adding extra nickel will shift the equilibrium to the right.
Ni (s) + 4CO (g) ⇔ Ni(CO)4 (g)

Accepted Answer

A) True 
 B)False

Question 19

Predict the shift in the direction of the reaction for the following chemical reaction:   + ultraviolet light     a) if oxygen (   ) is added.
b) if ozone (   ) is removed.
c) if oxygen (   ) is removed.
d) if more ultraviolet light is added.

Accepted Answer

a) shift right
b) sh

Question 20

For the following reaction at 1500 K, the equilibrium concentrations of each species are,   [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04.
N₂H₄ (g) ⇔ 2 H₂ (g) + N₂ (g)

Accepted Answer

A) True 
 B)False

For which of the following values of an equilibrium constant, Keq, would you expect the equilibrium to lie farthest to the right?

If the solubility of copper(II) sulfate is 4.9 × 10^-3 M, the solubility product is ________.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -L? (g) + H? (g) 2 HI (g)

For the following reaction, the equilibrium constant, Keq, is equal to 53.3. What is the concentration of I₂ at equilibrium, if the concentrations of HI and H₂ are 0.212 M and 1.576 M, respectively? H₂ + I₂ 2HI

For the following exothermic reaction: CO + OH predict the direction of the reaction if: a) temperature is decreased with the concentrations remaining the same. b) a catalyst is added with the concentrations AND temperature remaining the same. c) the concentration of is halved.

Decreasing the volume will ________. 2SO₃ (g) + 2CL₂ (g) 2SO₂CL₂ (g) + O₂ (g)

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N? (g)+ 2 H? (g) N?H? (g) [H?] = 0.20 M, [N?] = 0.10 M, [N?H?] = 0.10 M

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -2356.3

If the value of the equilibrium constant for the reverse reaction is 2.5 × 10^-6, the value of the equilibrium constant for the forward reaction is ________.

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCl₃] = 0.45 M and [PCl₅] = 0.73 M. Based on the calculated value of the equilibrium constant, the reaction is ________. CL₂ (g) + PCL₃ (g) PCl₅ (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -4.23

Reducing the pressure will shift the equilibrium to the left. N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Increasing the pressure will ________. 2 HCl (g) CL₂ (g) + H₂ (g)

If oxygen is removed this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

For the following exothermic reaction, what condition will increase the yield of product? C₂H₂ (g) + H₂O (g) CH₃CHO (g)

The equilibrium concentrations for the reaction at 673 K are [H₂] = 0.63 M, [N₂] = 0.45 M, and [NH₃] = 0.24 M. The value of Keq is ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

Adding extra nickel will shift the equilibrium to the right. Ni (s) + 4CO (g) ⇔ Ni(CO)4 (g)

Predict the shift in the direction of the reaction for the following chemical reaction: + ultraviolet light a) if oxygen ( ) is added. b) if ozone ( ) is removed. c) if oxygen ( ) is removed. d) if more ultraviolet light is added.

For the following reaction at 1500 K, the equilibrium concentrations of each species are, [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04. N₂H₄ (g) ⇔ 2 H₂ (g) + N₂ (g)

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces - the Ideal Gas

Solutions

When Reactants Turn Into Products

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

Exam 14: Chemical Equilibrium

For which of the following values of an equilibrium constant, Keq, would you expect the equilibrium to lie farthest to the right?

If the solubility of copper(II) sulfate is 4.9 × 10-3 M, the solubility product is ________.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -L? (g) + H? (g) 2 HI (g)

For the following reaction, the equilibrium constant, Keq, is equal to 53.3. What is the concentration of I₂ at equilibrium, if the concentrations of HI and H2 are 0.212 M and 1.576 M, respectively? H₂ + I₂ 2HI

For the following exothermic reaction: CO + OH predict the direction of the reaction if: a) temperature is decreased with the concentrations remaining the same. b) a catalyst is added with the concentrations AND temperature remaining the same. c) the concentration of is halved.

Decreasing the volume will ________. 2SO₃ (g) + 2CL₂ (g) 2SO₂CL₂ (g) + O₂ (g)

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N? (g)+ 2 H? (g) N?H? (g) [H?] = 0.20 M, [N?] = 0.10 M, [N?H?] = 0.10 M

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -2356.3

If the value of the equilibrium constant for the reverse reaction is 2.5 × 10-6, the value of the equilibrium constant for the forward reaction is ________.

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCl3] = 0.45 M and [PCl5] = 0.73 M. Based on the calculated value of the equilibrium constant, the reaction is ________. CL₂ (g) + PCL₃ (g) PCl5 (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -4.23

Reducing the pressure will shift the equilibrium to the left. N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Increasing the pressure will ________. 2 HCl (g) CL₂ (g) + H₂ (g)

If oxygen is removed this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

For the following exothermic reaction, what condition will increase the yield of product? C₂H₂ (g) + H₂O (g) CH₃CHO (g)

The equilibrium concentrations for the reaction at 673 K are [H₂] = 0.63 M, [N₂] = 0.45 M, and [NH₃] = 0.24 M. The value of Keq is ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

Adding extra nickel will shift the equilibrium to the right. Ni (s) + 4CO (g) ⇔ Ni(CO)4 (g)

Predict the shift in the direction of the reaction for the following chemical reaction: + ultraviolet light a) if oxygen ( ) is added. b) if ozone ( ) is removed. c) if oxygen ( ) is removed. d) if more ultraviolet light is added.

For the following reaction at 1500 K, the equilibrium concentrations of each species are, [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04. N₂H₄ (g) ⇔ 2 H₂ (g) + N₂ (g)

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces - the Ideal Gas

Solutions

When Reactants Turn Into Products

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

If the solubility of copper(II) sulfate is 4.9 × 10^-3 M, the solubility product is ________.

For the following reaction, the equilibrium constant, Keq, is equal to 53.3. What is the concentration of I₂ at equilibrium, if the concentrations of HI and H₂ are 0.212 M and 1.576 M, respectively? H₂ + I₂ 2HI

If the value of the equilibrium constant for the reverse reaction is 2.5 × 10^-6, the value of the equilibrium constant for the forward reaction is ________.

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCl₃] = 0.45 M and [PCl₅] = 0.73 M. Based on the calculated value of the equilibrium constant, the reaction is ________. CL₂ (g) + PCL₃ (g) PCl₅ (g)