Question 1

Consider the reaction: C (s) + CO? (g)   2 CO (g) (endothermic). 
Match each equilibrium change with its corresponding consequence.
-adding extra carbon dioxide

Accepted Answer

A) Equilibrium is shifted to the right. 
B) No effect on the equilibrium. 
C) Equilibrium is shifted to the left. 
A) Equilibrium is shifted to the right. 
B) No effect on the equilibrium. 
C) Equilibrium is shifted to the left. A

Question 2

The equilibrium constant is equal to which of the following?

Accepted Answer

A)  kforward / kreverse 
B)  kreverse / kforward 
C)  kforward × kreverse 
D)  1 / (kforward/kreverse) 
A)  kforward / kreverse 
B)  kreverse / kforward 
C)  kforward × kreverse 
D)  1 / (kforward/kreverse) A

Question 3

Expanding the reaction vessel will shift the equilibrium to the right.
3O₂ (g) ⇔ 2O₃ (g)

Accepted Answer

A) True 
 B)False  False

Question 4

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-4.5 × 10-2

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 5

At equilibrium, the concentrations of reactants and products are always exactly the same.

Accepted Answer

A) True 
 B)False

Question 6

Write an expression for the equilibrium constant (Keq) for the following reaction.   (g) +   (g)     (g) + NO (g)

Accepted Answer

Keq = [ @#IMG-DLM& ]

Question 7

Adding helium to the reaction vessel will ________. 2H₂S (g) + 3O₂ (g)   2SO₂ (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 8

Increasing the volume of the system will ________. 2H₂S (g) + 3O₂ (g)   2SO₂ (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 9

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-3.7 × 103

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 10

Consider the reaction: C (s) + CO? (g)   2 CO (g) (endothermic). 
Match each equilibrium change with its corresponding consequence.
-adding extra carbon

Accepted Answer

A) Equilibrium is shifted to the right. 
B) No effect on the equilibrium. 
C) Equilibrium is shifted to the left. 
A) Equilibrium is shifted to the right. 
B) No effect on the equilibrium. 
C) Equilibrium is shifted to the left.

Question 11

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-2 NH? (g)   N? (g) + 3 H? (g)

Accepted Answer

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

Question 12

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

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 13

If more     is added to the following reaction already at equilibrium:         what would be expected to happen to the rate of the forward reaction?

Accepted Answer

Forward reaction rat

Question 14

Reducing the pressure will shift the equilibrium to the right.
N₂ (g) + O₂ (g) ⇔ 2NO (g)

Accepted Answer

A) True 
 B)False

Question 15

Decreasing the concentration of nitrogen will shift the equilibrium to the left.
N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Accepted Answer

A) True 
 B)False

Question 16

Predict the shift in the direction of the reaction for the following chemical reaction:   (g) +   (g)     (g)+   O (g)
a) if methane (   ) is added
b) if carbon dioxide (   ) is added
c) if water (   O) is removed

Accepted Answer

a) shift r

Question 17

Which of the following statements is true for a chemical reaction that has not reached an equilibrium?

Accepted Answer

A)  The "reverse" reaction rate is zero. 
B)  The "forward" reaction rate is zero. 
C)  The "forward" and "reverse" reaction rates are equal. 
D)  Both A and B are true statements. 
E)  None of the above are true statements. 
A)  The "reverse" reaction rate is zero. 
B)  The "forward" reaction rate is zero. 
C)  The "forward" and "reverse" reaction rates are equal. 
D)  Both A and B are true statements. 
E)  None of the above are true statements.

Question 18

If a chemical reaction at an equilibrium state is disturbed, the reaction will compensate for the disturbance in some way so that equilibrium can be restored.

Accepted Answer

A) True 
 B)False

Question 19

Adding excess oxygen 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 not known 
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 not known

Question 20

Which of the following will shift the reaction to the right? CH₄ (g) + 2O₂ (g)   CO₂ (g) + 2H₂O (g)

Accepted Answer

A)  adding excess oxygen 
B)  removing carbon dioxide as soon as it is formed 
C)  increasing the pressure 
D)  both A and B 
A)  adding excess oxygen 
B)  removing carbon dioxide as soon as it is formed 
C)  increasing the pressure 
D)  both A and B

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic). Match each equilibrium change with its corresponding consequence. -adding extra carbon dioxide

The equilibrium constant is equal to which of the following?

Expanding the reaction vessel will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -4.5 × 10^-2

At equilibrium, the concentrations of reactants and products are always exactly the same.

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) + (g) (g) + NO (g)

Adding helium to the reaction vessel will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Increasing the volume of the system will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -3.7 × 10³

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic). Match each equilibrium change with its corresponding consequence. -adding extra carbon

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 NH? (g) N? (g) + 3 H? (g)

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

If more is added to the following reaction already at equilibrium: what would be expected to happen to the rate of the forward reaction?

Reducing the pressure will shift the equilibrium to the right. N₂ (g) + O₂ (g) ⇔ 2NO (g)

Decreasing the concentration of nitrogen will shift the equilibrium to the left. N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Predict the shift in the direction of the reaction for the following chemical reaction: (g) + (g) (g)+ O (g) a) if methane ( ) is added b) if carbon dioxide ( ) is added c) if water ( O) is removed

Which of the following statements is true for a chemical reaction that has not reached an equilibrium?

If a chemical reaction at an equilibrium state is disturbed, the reaction will compensate for the disturbance in some way so that equilibrium can be restored.

Adding excess oxygen will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

Which of the following will shift the reaction to the right? CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (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

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic). Match each equilibrium change with its corresponding consequence. -adding extra carbon dioxide

The equilibrium constant is equal to which of the following?

Expanding the reaction vessel will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -4.5 × 10-2

At equilibrium, the concentrations of reactants and products are always exactly the same.

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) + (g) (g) + NO (g)

Adding helium to the reaction vessel will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Increasing the volume of the system will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -3.7 × 103

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic). Match each equilibrium change with its corresponding consequence. -adding extra carbon

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 NH? (g) N? (g) + 3 H? (g)

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

If more is added to the following reaction already at equilibrium: what would be expected to happen to the rate of the forward reaction?

Reducing the pressure will shift the equilibrium to the right. N₂ (g) + O₂ (g) ⇔ 2NO (g)

Decreasing the concentration of nitrogen will shift the equilibrium to the left. N₂ (g) + 2O₂ (g) ⇔ 2NO₂ (g)

Predict the shift in the direction of the reaction for the following chemical reaction: (g) + (g) (g)+ O (g) a) if methane ( ) is added b) if carbon dioxide ( ) is added c) if water ( O) is removed

Which of the following statements is true for a chemical reaction that has not reached an equilibrium?

If a chemical reaction at an equilibrium state is disturbed, the reaction will compensate for the disturbance in some way so that equilibrium can be restored.

Adding excess oxygen will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

Which of the following will shift the reaction to the right? CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (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

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -4.5 × 10^-2

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -3.7 × 10³