Question 1

Increasing the pressure 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 2

Oxygen (O₂) and ozone (O₃) coexist in the stratosphere and are in equilibrium with one another:       a) Assuming that no other factors affect this equilibrium, if ozone (   ) is being "depleted" (somehow removed from the reaction system entirely), what is the direction of the equilibrium shift?
b) What must be happening to the concentration of oxygen (   ) as a result of the equilibrium shift predicted in part a?

Accepted Answer

a) With no other factors, equi

Question 3

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-2 NH? (g)   N? (g) + 3 H? (g)

Accepted Answer

A) no effect 
B) right (?) 
C) left (?) 
A) no effect 
B) right (?) 
C) left (?)

Question 4

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

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 5

Adding iron(III) chloride will ________. FeCL₃ (aq) + KSCN (aq)   3[Fe(SCN)6] (aq) + 3KCl (aq)
Yellow colorless red colorless

Accepted Answer

A)  turn the solution more red. 
B)  turn the solution less red. 
C)  turn the solution clear. 
D)  have no effect on the color. 
A)  turn the solution more red. 
B)  turn the solution less red. 
C)  turn the solution clear. 
D)  have no effect on the color.

Question 6

The following chemical reaction has reached equilibrium.     (g)     (g) Calculate the equilibrium constant, Keq, if the concentrations of     and   are 0.0238 M and 0.196 M, respectively.

Accepted Answer

A)  8.34 
B)  346 
C)  0.621 
D)  1.61 
A)  8.34 
B)  346 
C)  0.621 
D)  1.61

Question 7

In an endothermic 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 8

The following chemical reaction has reached equilibrium. 2NO (g) + O₂ (g)   2NO₂ (g)
Calculate the equilibrium constant, Keq, if the concentrations of reactants and products are 1.26 × 10-10 M for NO, 2.28 × 10-3 M for O₂, and 9.32 × 10-6 M for NO₂.

Accepted Answer

A)  2.40 × 10-12 
B)  3.28 × 10-7  
C)  2.61 × 10-17 
D)  2.40 × 1012 
A)  2.40 × 10-12 
B)  3.28 × 10-7  
C)  2.61 × 10-17 
D)  2.40 × 1012

Question 9

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-O₂ (g) + 2F₂ (g)   2 OF₂ (g)

Accepted Answer

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

Question 10

Predict the direction in which the reaction will shift for the following reactions if the temperature is increased:
a) CO +       +   O (exothermic)
b)   +     2HI (endothermic)
c) CO +   O     +   (exothermic)

Accepted Answer

a) shift to the left

Question 11

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-L₂ (g) + H₂ (g)   2 HI (g)

Accepted Answer

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

Question 12

Consider the reaction: C (s) + CO? (g)   2 CO (g) (endothermic). 
Match each equilibrium change with its corresponding consequence.
-increasing 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 13

The equilibrium constant expression for the reaction is ________. N₂ (g) + 3H₂ (g)   2NH₃ (g)

Accepted Answer

A)  Keq = [N₂] [3H₂]3 / [2NH₃]2 
B)  Keq = [NH₃]2 / [N₂] [H₂]3 
C)  Keq = [N₂] [H₂]3 / [NH₃]2 
D)  Keq = [2NH₃]2 / [N₂] [3H₂]3 
A)  Keq = [N₂] [3H₂]3 / [2NH₃]2 
B)  Keq = [NH₃]2 / [N₂] [H₂]3 
C)  Keq = [N₂] [H₂]3 / [NH₃]2 
D)  Keq = [2NH₃]2 / [N₂] [3H₂]3

Question 14

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

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 15

The term "molar solubility of a salt" refers to the molar concentration of one anion (or cation) formed in an aqueous, saturated solution of that salt.

Accepted Answer

A) True 
 B)False

Question 16

Which of the following will shift the equilibrium to the left? 2H₂S (g) + 3O₂ (g)   2SO₂ (g) + 2H₂O (g)

Accepted Answer

A)  adding sulfur dioxide 
B)  adding hydrogen sulfide 
C)  decreasing the pressure 
D)  both A and C 
A)  adding sulfur dioxide 
B)  adding hydrogen sulfide 
C)  decreasing the pressure 
D)  both A and C

Question 17

Adding a couple of drops of an aqueous KCl solution will ________. FeCL₃ (aq) + KSCN (aq)   K3[Fe(SCN)6] (aq) + 3KCl (aq)
Yellow colorless red colorless

Accepted Answer

A)  turn the solution more red. 
B)  turn the solution less red. 
C)  turn the solution clear. 
D)  have no effect on the color. 
A)  turn the solution more red. 
B)  turn the solution less red. 
C)  turn the solution clear. 
D)  have no effect on the color.

Question 18

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-2 C?H?? (g) + 25 O?

Accepted Answer

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

Question 19

Predict the direction in which the reaction will shift for the following reactions if the temperature is decreased:
a)   + NO     +   (endothermic)
b)   +   O   CO +   (endothermic)
c)   +       (exothermic)

Accepted Answer

a) shift l

Question 20

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-6.2 × 1010

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

Increasing the pressure will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 NH? (g) N? (g) + 3 H? (g)

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

Adding iron(III) chloride will ________. FeCL₃ (aq) + KSCN (aq) 3[Fe(SCN)6] (aq) + 3KCl (aq) Yellow colorless red colorless

The following chemical reaction has reached equilibrium. (g) (g) Calculate the equilibrium constant, Keq, if the concentrations of and are 0.0238 M and 0.196 M, respectively.

In an endothermic reaction, adding heat will ________.

The following chemical reaction has reached equilibrium. 2NO (g) + O₂ (g) 2NO₂ (g) Calculate the equilibrium constant, Keq, if the concentrations of reactants and products are 1.26 × 10^-10 M for NO, 2.28 × 10^-3 M for O₂, and 9.32 × 10^-6 M for NO₂.

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -O₂ (g) + 2F₂ (g) 2 OF₂ (g)

Predict the direction in which the reaction will shift for the following reactions if the temperature is increased: a) CO + + O (exothermic) b) + 2HI (endothermic) c) CO + O + (exothermic)

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -L₂ (g) + H₂ (g) 2 HI (g)

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

The equilibrium constant expression for the reaction is ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

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

The term "molar solubility of a salt" refers to the molar concentration of one anion (or cation) formed in an aqueous, saturated solution of that salt.

Which of the following will shift the equilibrium to the left? 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Adding a couple of drops of an aqueous KCl solution will ________. FeCL₃ (aq) + KSCN (aq) K3[Fe(SCN)6] (aq) + 3KCl (aq) Yellow colorless red colorless

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 C?H?? (g) + 25 O?

Predict the direction in which the reaction will shift for the following reactions if the temperature is decreased: a) + NO + (endothermic) b) + O CO + (endothermic) c) + (exothermic)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -6.2 × 10¹⁰

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

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Exam 14: Chemical Equilibrium

Increasing the pressure will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 NH? (g) N? (g) + 3 H? (g)

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

Adding iron(III) chloride will ________. FeCL₃ (aq) + KSCN (aq) 3[Fe(SCN)6] (aq) + 3KCl (aq) Yellow colorless red colorless

The following chemical reaction has reached equilibrium. (g) (g) Calculate the equilibrium constant, Keq, if the concentrations of and are 0.0238 M and 0.196 M, respectively.

In an endothermic reaction, adding heat will ________.

The following chemical reaction has reached equilibrium. 2NO (g) + O₂ (g) 2NO₂ (g) Calculate the equilibrium constant, Keq, if the concentrations of reactants and products are 1.26 × 10-10 M for NO, 2.28 × 10-3 M for O₂, and 9.32 × 10-6 M for NO₂.

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -O₂ (g) + 2F₂ (g) 2 OF₂ (g)

Predict the direction in which the reaction will shift for the following reactions if the temperature is increased: a) CO + + O (exothermic) b) + 2HI (endothermic) c) CO + O + (exothermic)

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -L₂ (g) + H₂ (g) 2 HI (g)

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

The equilibrium constant expression for the reaction is ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

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

The term "molar solubility of a salt" refers to the molar concentration of one anion (or cation) formed in an aqueous, saturated solution of that salt.

Which of the following will shift the equilibrium to the left? 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Adding a couple of drops of an aqueous KCl solution will ________. FeCL₃ (aq) + KSCN (aq) K3[Fe(SCN)6] (aq) + 3KCl (aq) Yellow colorless red colorless

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 C?H?? (g) + 25 O?

Predict the direction in which the reaction will shift for the following reactions if the temperature is decreased: a) + NO + (endothermic) b) + O CO + (endothermic) c) + (exothermic)

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -6.2 × 1010

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

The following chemical reaction has reached equilibrium. 2NO (g) + O₂ (g) 2NO₂ (g) Calculate the equilibrium constant, Keq, if the concentrations of reactants and products are 1.26 × 10^-10 M for NO, 2.28 × 10^-3 M for O₂, and 9.32 × 10^-6 M for NO₂.

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -6.2 × 10¹⁰