Question 1

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-2 SO₃ (g) + 2 CL₂ (g)

Accepted Answer

A) no effect 
B) right (→) 
C) left (←) 
A) no effect 
B) right (→) 
C) left (←)

Question 2

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Accepted Answer

A) True 
 B)False

Question 3

Removing ozone as soon as it is formed will shift the equilibrium to the right.
3O₂ (g) ⇔ 2O₃ (g)

Accepted Answer

A) True 
 B)False

Question 4

Calculate the equilibrium concentration of N₂ for the following reaction.   +       The equilibrium constant Keq is 0.055 and the concentrations of   and   are 1.20 M and 0.225 M, respectively.

Accepted Answer

A)  0.0915 M 
B)  0.533 M 
C)  0.915 M 
D)  3.41 M 
A)  0.0915 M 
B)  0.533 M 
C)  0.915 M 
D)  3.41 M

Question 5

Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

Accepted Answer

A)  The rate increases as equilibrium is approached. 
B)  The rate decreases as equilibrium is approached. 
C)  The rate remains constant. 
D)  The rate slows down, then increases, as equilibrium is approached. 
A)  The rate increases as equilibrium is approached. 
B)  The rate decreases as equilibrium is approached. 
C)  The rate remains constant. 
D)  The rate slows down, then increases, as equilibrium is approached.

Question 6

Decreasing the concentration of ammonia gas will ________. 2NH₃ (g)   N₂ (g) + 3H₂ (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

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 8

If the solubility of calcium fluoride is 2.0 × 10-4 M, the solubility product value is ________.

Accepted Answer

A)  1.6 × 10-12 
B)  3.2 × 10-11 
C)  4.0 × 10-8 
D)  8.0 × 10-12 
A)  1.6 × 10-12 
B)  3.2 × 10-11 
C)  4.0 × 10-8 
D)  8.0 × 10-12

Question 9

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

Accepted Answer

A)  2.2 
B)  0.15 
C)  0.048 
D)  4.7 
A)  2.2 
B)  0.15 
C)  0.048 
D)  4.7

Question 10

For an endothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B 
A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B

Question 11

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

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 12

The solubility of SrF₂ in water (given Ksp = 2.6 × 10-9 ) is ________.

Accepted Answer

A)  4.3 × 10-4 M 
B)  1.2 × 10-4 M 
C)  7.6 × 10-5 M 
D)  8.7 × 10-4 M 
A)  4.3 × 10-4 M 
B)  1.2 × 10-4 M 
C)  7.6 × 10-5 M 
D)  8.7 × 10-4 M

Question 13

At equilibrium, the amount of product present is always greater than the amount of reactant present.

Accepted Answer

A) True 
 B)False

Question 14

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value.
-N?O5 (g)   2 O? (g) +   [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M

Accepted Answer

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

Question 15

If the reaction vessel is expanded, 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 16

Removing ammonia as soon as it is formed will ________. N₂ (g) + 3H₂ (g)   2NH₃ (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 17

In an exothermic reaction, adding heat will ________.

Accepted Answer

A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B 
A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B

Question 18

Removing product will ________. 2SO₂ (g) + O₂ (g)   2SO₃ (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 19

For an exothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B 
A)  increase the amount of products 
B)  decrease the amount of reactants 
C)  decrease the amount of products 
D)  both A and B

Question 20

Write an expression for the equilibrium constant (Keq) for the following reaction.
HCl (g) + H₂O (l)   H₃O+ (aq)+ Cl- (aq)

Accepted Answer

Keq = [ @#IMG-DLM& ]

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Removing ozone as soon as it is formed will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Calculate the equilibrium concentration of N₂ for the following reaction. + The equilibrium constant Keq is 0.055 and the concentrations of and are 1.20 M and 0.225 M, respectively.

Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

Decreasing the concentration of ammonia gas will ________. 2NH₃ (g) N₂ (g) + 3H₂ (g)

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

If the solubility of calcium fluoride is 2.0 × 10^-4 M, the solubility product value is ________.

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

For an endothermic reaction, lowering the temperature of the reaction will ________.

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

The solubility of SrF₂ in water (given Ksp = 2.6 × 10^-9 ) is ________.

At equilibrium, the amount of product present is always greater than the amount of reactant present.

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O₅ (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O₅] = 0.10 M

If the reaction vessel is expanded, this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

Removing ammonia as soon as it is formed will ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

In an exothermic reaction, adding heat will ________.

Removing product will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

For an exothermic reaction, lowering the temperature of the reaction will ________.

Write an expression for the equilibrium constant (Keq) for the following reaction. HCl (g) + H₂O (l) H₃O+ (aq)+ Cl- (aq)

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

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Removing ozone as soon as it is formed will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Calculate the equilibrium concentration of N₂ for the following reaction. + The equilibrium constant Keq is 0.055 and the concentrations of and are 1.20 M and 0.225 M, respectively.

Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

Decreasing the concentration of ammonia gas will ________. 2NH₃ (g) N₂ (g) + 3H₂ (g)

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

If the solubility of calcium fluoride is 2.0 × 10-4 M, the solubility product value is ________.

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

For an endothermic reaction, lowering the temperature of the reaction will ________.

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

The solubility of SrF₂ in water (given Ksp = 2.6 × 10-9 ) is ________.

At equilibrium, the amount of product present is always greater than the amount of reactant present.

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O5 (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M

If the reaction vessel is expanded, this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

Removing ammonia as soon as it is formed will ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

In an exothermic reaction, adding heat will ________.

Removing product will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

For an exothermic reaction, lowering the temperature of the reaction will ________.

Write an expression for the equilibrium constant (Keq) for the following reaction. HCl (g) + H₂O (l) H₃O+ (aq)+ Cl- (aq)

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 calcium fluoride is 2.0 × 10^-4 M, the solubility product value is ________.

The solubility of SrF₂ in water (given Ksp = 2.6 × 10^-9 ) is ________.

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O₅ (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O₅] = 0.10 M