Question 1

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-CH₄ (g) + 2 O₂ (g)

Accepted Answer

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

Question 2

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

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 3

Identify each of the equilibrium constant values  as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored."
-0.563

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 4

For this chemical reaction at equilibrium: N₂ (g) + 3H₂ (g)   2NH₃ (g)
Which of the following statements is true of the reaction rate?

Accepted Answer

A)  The forward rate is faster than the reverse rate. 
B)  The reverse rate is faster than the forward rate. 
C)  Both the forward and reverse rates are zero. 
D)  The forward and reverse rates are the same. 
A)  The forward rate is faster than the reverse rate. 
B)  The reverse rate is faster than the forward rate. 
C)  Both the forward and reverse rates are zero. 
D)  The forward and reverse rates are the same.

Question 5

For the following endothermic reaction, what condition will increase the yield of product? N₂ (g) + 2H₂ (g)   N₂H₄ (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 6

The solubility product expression for silver(I) sulfate is ________.

Accepted Answer

A)  Ksp = [Ag+] [SO₄-2] 
B)  Ksp = [2 Ag+] [SO₄-2] 
C)  Ksp = [Ag+]2[SO₄-2] 
D)  Ksp = [2Ag+]2[SO₄-2] 
A)  Ksp = [Ag+] [SO₄-2] 
B)  Ksp = [2 Ag+] [SO₄-2] 
C)  Ksp = [Ag+]2[SO₄-2] 
D)  Ksp = [2Ag+]2[SO₄-2]

Question 7

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-CH₄ (g) + 2 O₂ (g)

Accepted Answer

A) left (←) 
B) right (→) 
A) left (←) 
B) right (→)

Question 8

Write an expression for the equilibrium constant (Keq) for the following reaction.
NH₃ (g) + H₂O (l)     (aq) +   + (aq)

Accepted Answer

Keq = [ @#IMG-DLM& ]

Question 9

No reaction exists in which 100% of the reactants are consumed.

Accepted Answer

A) True 
 B)False

Question 10

Adding more oxygen 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 11

The equilibrium condition of a chemical reaction is not related to temperature.

Accepted Answer

A) True 
 B)False

Question 12

Adding a catalyst will ________. FeCL₃ + KSCN   K3[Fe(SCN)6] + 3KCl
Yellow colorless red colorless

Accepted Answer

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

Question 13

Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________. A + 3B   2C

Accepted Answer

A)  [A]  [B] 
C)  [A] = [B] 
D)  One cannot say unless the equilibrium constant value is known. 
A)  [A]  [B] 
C)  [A] = [B] 
D)  One cannot say unless the equilibrium constant value is known.

Question 14

Removing sulfur dioxide as it is formed 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 15

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-2 SO₃ (g) + 2 CL₂ (g)

Accepted Answer

A) left (←) 
B) right (→) 
A) left (←) 
B) right (→)

Question 16

The concentrations of reactants and products do not change as equilibrium is approached, only the rate at which products are formed and reactants are consumed.

Accepted Answer

A) True 
 B)False

Question 17

Consider the reaction with Kc = 0.211. Which of the following pairs of concentrations indicate that the system is not at equilibrium? N₂O₄ (g)   2NO₂ (g)

Accepted Answer

A)  [N₂O₄] = 0.00140 M; [NO₂] = 0.0172 M 
B)  [N₂O₄] = 0.00280 M; [NO₂] = 0.0243 M 
C)  [N₂O₄] = 0.00452 M; [NO₂] = 0.0309 M 
D)  [N₂O₄] = 0.00840 M; [NO₂] = 0.0572 M 
A)  [N₂O₄] = 0.00140 M; [NO₂] = 0.0172 M 
B)  [N₂O₄] = 0.00280 M; [NO₂] = 0.0243 M 
C)  [N₂O₄] = 0.00452 M; [NO₂] = 0.0309 M 
D)  [N₂O₄] = 0.00840 M; [NO₂] = 0.0572 M

Question 18

A product favored reaction has Keq = 1.

Accepted Answer

A) True 
 B)False

Question 19

Increasing the pressure 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 20

Write an expression for the equilibrium constant (Keq) for the following reaction.   (g)     (g)

Accepted Answer

The answer of Write an expression for the equilibrium constant...

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -CH₄ (g) + 2 O₂ (g)

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

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -0.563

For this chemical reaction at equilibrium: N₂ (g) + 3H₂ (g) 2NH₃ (g) Which of the following statements is true of the reaction rate?

For the following endothermic reaction, what condition will increase the yield of product? N₂ (g) + 2H₂ (g) N₂H₄ (g)

The solubility product expression for silver(I) sulfate is ________.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -CH₄ (g) + 2 O₂ (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. NH₃ (g) + H₂O (l) (aq) + + (aq)

No reaction exists in which 100% of the reactants are consumed.

Adding more oxygen will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

The equilibrium condition of a chemical reaction is not related to temperature.

Adding a catalyst will ________. FeCL₃ + KSCN K3[Fe(SCN)6] + 3KCl Yellow colorless red colorless

Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________. A + 3B 2C

Removing sulfur dioxide as it is formed will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

The concentrations of reactants and products do not change as equilibrium is approached, only the rate at which products are formed and reactants are consumed.

Consider the reaction with Kc = 0.211. Which of the following pairs of concentrations indicate that the system is not at equilibrium? N₂O₄ (g) 2NO₂ (g)

A product favored reaction has Keq = 1.

Increasing the pressure will ________. 2NH₃ (g) N₂ (g) + 3H₂ (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) (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

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Exam 14: Chemical Equilibrium

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -CH₄ (g) + 2 O₂ (g)

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

Identify each of the equilibrium constant values as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored." -0.563

For this chemical reaction at equilibrium: N₂ (g) + 3H₂ (g) 2NH₃ (g) Which of the following statements is true of the reaction rate?

For the following endothermic reaction, what condition will increase the yield of product? N₂ (g) + 2H₂ (g) N₂H₄ (g)

The solubility product expression for silver(I) sulfate is ________.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -CH₄ (g) + 2 O₂ (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. NH₃ (g) + H₂O (l) (aq) + + (aq)

No reaction exists in which 100% of the reactants are consumed.

Adding more oxygen will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

The equilibrium condition of a chemical reaction is not related to temperature.

Adding a catalyst will ________. FeCL₃ + KSCN K3[Fe(SCN)6] + 3KCl Yellow colorless red colorless

Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________. A + 3B 2C

Removing sulfur dioxide as it is formed will ________. 2H₂S (g) + 3O₂ (g) 2SO₂ (g) + 2H₂O (g)

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

The concentrations of reactants and products do not change as equilibrium is approached, only the rate at which products are formed and reactants are consumed.

Consider the reaction with Kc = 0.211. Which of the following pairs of concentrations indicate that the system is not at equilibrium? N₂O₄ (g) 2NO₂ (g)

A product favored reaction has Keq = 1.

Increasing the pressure will ________. 2NH₃ (g) N₂ (g) + 3H₂ (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) (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