Question 1

Consider the equilibrium system   If C is removed, the equilibrium will ____, and if CO is added, the equilibrium will ____.

Accepted Answer

A)  shift to the left; shift to the left 
B)  shift to the right; shift to the right 
C)  shift to the right; shift to the left 
D)  be unchanged; shift to the left 
E)  be unchanged; shift to the right 
A)  shift to the left; shift to the left 
B)  shift to the right; shift to the right 
C)  shift to the right; shift to the left 
D)  be unchanged; shift to the left 
E)  be unchanged; shift to the right

Question 2

In a balanced chemical equation, if there is no net change in the total number of moles of gas from the reactant side to the product side, then

Accepted Answer

A)  Kp = 1.00 
B)  Kp = Kc 
C)  Kc = 1.00 
D)  at equilibrium, the reaction has gone to 50% completion 
E)  all of these 
A)  Kp = 1.00 
B)  Kp = Kc 
C)  Kc = 1.00 
D)  at equilibrium, the reaction has gone to 50% completion 
E)  all of these

Question 3

If the reaction quotient, Q, is greater than the equilibrium constant, K, then

Accepted Answer

A)  the forward reaction must be favored 
B)  the reaction will proceed in the forward direction 
C)  the reaction has gone to 100% completion and is at equilibrium 
D)  the reaction has not yet started in the forward direction 
E)  the reaction will proceed in the reverse direction 
A)  the forward reaction must be favored 
B)  the reaction will proceed in the forward direction 
C)  the reaction has gone to 100% completion and is at equilibrium 
D)  the reaction has not yet started in the forward direction 
E)  the reaction will proceed in the reverse direction

Question 4

Which of the following is not true for equilibrium constants?

Accepted Answer

A)  when related reactions are added together, their equilibrium constants are added together 
B)  the equilibrium constants of the forward and reverse reactions are negative reciprocals of one another 
C)  when the coefficients in a balanced chemical reaction are multiplied by a factor, the equilibrium constant is multiplied by the same factor 
D)  the equilibrium constants of the forward and reverse reactions are equal to the respective rate constants of these reactions 
E)  all of these 
A)  when related reactions are added together, their equilibrium constants are added together 
B)  the equilibrium constants of the forward and reverse reactions are negative reciprocals of one another 
C)  when the coefficients in a balanced chemical reaction are multiplied by a factor, the equilibrium constant is multiplied by the same factor 
D)  the equilibrium constants of the forward and reverse reactions are equal to the respective rate constants of these reactions 
E)  all of these

Question 5

For an exothermic reaction, an increase in temperature

Accepted Answer

A)  always means an increase in Kc 
B)  always means a decrease in Kc 
C)  the reaction will become more product-favored at higher temperatures 
D)  the reaction will become more reactant-favored at higher temperatures 
E)  both b and d 
A)  always means an increase in Kc 
B)  always means a decrease in Kc 
C)  the reaction will become more product-favored at higher temperatures 
D)  the reaction will become more reactant-favored at higher temperatures 
E)  both b and d

Question 6

For the reaction  Kc = 1.37. If the concentrations of A and B are equal, what is the value of that concentration?

Accepted Answer

A)  0.685 M 
B)  0.822 M 
C)  1.17 M 
D)  1.37 M 
E)  1.88 M 
A)  0.685 M 
B)  0.822 M 
C)  1.17 M 
D)  1.37 M 
E)  1.88 M

Question 7

If the value of Kc for a given reaction at a given temperature is a large number, the energy of the products is likely to be ____ the energy of the reactants because ____.

Accepted Answer

A)  greater than; the value of Kc favors the reactants 
B)  less than; the value of Kc favors the reactants 
C)  the same as; the value of Kc favors neither the products nor the reactants 
D)  greater than; the value of Kc favors the products 
E)  less than; the value of Kc favors the products 
A)  greater than; the value of Kc favors the reactants 
B)  less than; the value of Kc favors the reactants 
C)  the same as; the value of Kc favors neither the products nor the reactants 
D)  greater than; the value of Kc favors the products 
E)  less than; the value of Kc favors the products

Question 8

The equilibrium for a particular chemical reaction is dependent on the

Accepted Answer

A)  homogeneous catalyst concentration, if catalyst is present 
B)  direction of approach 
C)  temperature of the reaction 
D)  atmospheric pressure 
E)  initial concentrations of the reactants 
A)  homogeneous catalyst concentration, if catalyst is present 
B)  direction of approach 
C)  temperature of the reaction 
D)  atmospheric pressure 
E)  initial concentrations of the reactants

Question 9

Consider the reaction
   for which Kp = 2.00 at 20$\circ$C. A mixture of NO(g) at a partial pressure of 1.50 atm and NO2(g) at a partial pressure of 0.50 atm is allowed to come to equilibrium in a sealed container maintained at 20$\circ$C. What is the total pressure now?
The expression for 
  .

Accepted Answer

Set up the reaction table as described i

Question 10

Consider the equilibrium reaction   A sample of pure NO2(g) of concentration 0.140 M is allowed to come to equilibrium. It is then found that 57.0 % of the NO2(g) has reacted to form N2O4(g). What is the value of Kc?

Accepted Answer

A)  0.211 
B)  0.377 
C)  0.754 
D)  4.73 
E)  11.0 
A)  0.211 
B)  0.377 
C)  0.754 
D)  4.73 
E)  11.0

Question 11

Consider the gas-phase equilibrium A   B. In a series of experiments, different initial amounts of A and B are mixed together, and the mixture in each case allowed to come to equilibrium. Which one of these experiments would yield values for the amounts of A and B present at equilibrium different from all the other experiments?

Accepted Answer

A)  3.0 moles A, 4.5 moles B 
B)  4.5 moles A, 3.0 moles B 
C)  1.5 moles A, 4.5 moles B 
D)  7.5 moles A, no B 
E)  0.5 moles A, 7.0 moles B 
A)  3.0 moles A, 4.5 moles B 
B)  4.5 moles A, 3.0 moles B 
C)  1.5 moles A, 4.5 moles B 
D)  7.5 moles A, no B 
E)  0.5 moles A, 7.0 moles B

Question 12

Which of the following is false?

Accepted Answer

A)  a large equilibrium constant is indicative of a reactant-favored reaction 
B)  an equilibrium constant close to 1.00 always indicates a highly product-favored reaction 
C)  if Kp = Kc the reaction has gone to 100% completion at equilibrium 
D)  if Kp = Kc = 0.50, the reaction has gone to 50% completion at equilibrium 
E)  all of these 
A)  a large equilibrium constant is indicative of a reactant-favored reaction 
B)  an equilibrium constant close to 1.00 always indicates a highly product-favored reaction 
C)  if Kp = Kc the reaction has gone to 100% completion at equilibrium 
D)  if Kp = Kc = 0.50, the reaction has gone to 50% completion at equilibrium 
E)  all of these

Question 13

Which of the following is true for an equilibrium system?

Accepted Answer

A)  in an equilibrium system, molecules that are higher in energy occur less often 
B)  if there are more product molecules than reactant molecules, entropy favors the products in an equilibrium system 
C)  the higher the temperature is, the less important the energy effect (DH) becomes 
D)  the higher the temperature is, the more the entropy effect (dispersal of energy) determines the position of equilibrium 
E)  all of these 
A)  in an equilibrium system, molecules that are higher in energy occur less often 
B)  if there are more product molecules than reactant molecules, entropy favors the products in an equilibrium system 
C)  the higher the temperature is, the less important the energy effect (DH) becomes 
D)  the higher the temperature is, the more the entropy effect (dispersal of energy) determines the position of equilibrium 
E)  all of these

Question 14

A particular reaction mixture (Kp = 10) consisting of both gaseous reactants and products is analyzed and is determined to have a value of Q = 15. The pressure of the reaction mixture is then doubled by the addition of argon gas and the reaction is allowed to proceed to equilibrium. At equilibrium

Accepted Answer

A) Kp > 10 B) Q = 15 C) Q = 10 D) Kp < 10 E) Q = 30 A) Kp > 10 B) Q = 15 C) Q = 10 D) Kp < 10 E) Q = 30

Question 15

Consider the gas-phase equilibrium A   B. Certain amounts of A and B are mixed in a vessel. As they come to equilibrium

Accepted Answer

A)  the forward reaction rate declines and the reverse reaction rate rises. 
B)  the reverse reaction rate declines and the forward reaction rate rises. 
C)  both forward and reverse reaction rates decline. 
D)  both forward and reverse reaction rates rise. 
E)  either a or b, but we cannot say which without more information. 
A)  the forward reaction rate declines and the reverse reaction rate rises. 
B)  the reverse reaction rate declines and the forward reaction rate rises. 
C)  both forward and reverse reaction rates decline. 
D)  both forward and reverse reaction rates rise. 
E)  either a or b, but we cannot say which without more information.

Question 16

If a catalyst is added to a chemical reaction, the equilibrium yield of a product will be ____, and the time taken to come to equilibrium will be ____ than before.

Accepted Answer

A)  higher; less 
B)  lower; the same 
C)  higher; the same 
D)  the same; less 
E)  lower; less 
A)  higher; less 
B)  lower; the same 
C)  higher; the same 
D)  the same; less 
E)  lower; less

Question 17

The equilibrium constant expression for the reverse of the reaction given below is

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Consider the equilibrium system If C is removed, the equilibrium will , and if CO is added, the equilibrium will .

In a balanced chemical equation, if there is no net change in the total number of moles of gas from the reactant side to the product side, then

If the reaction quotient, Q, is greater than the equilibrium constant, K, then

Which of the following is not true for equilibrium constants?

For an exothermic reaction, an increase in temperature

For the reaction K_c = 1.37. If the concentrations of A and B are equal, what is the value of that concentration?

If the value of K_c for a given reaction at a given temperature is a large number, the energy of the products is likely to be the energy of the reactants because .

The equilibrium for a particular chemical reaction is dependent on the

Consider the equilibrium reaction A sample of pure NO₂(g) of concentration 0.140 M is allowed to come to equilibrium. It is then found that 57.0 % of the NO₂(g) has reacted to form N₂O₄(g). What is the value of K_c?

Which of the following is false?

Which of the following is true for an equilibrium system?

A particular reaction mixture (K_p = 10) consisting of both gaseous reactants and products is analyzed and is determined to have a value of Q = 15. The pressure of the reaction mixture is then doubled by the addition of argon gas and the reaction is allowed to proceed to equilibrium. At equilibrium

Consider the gas-phase equilibrium A B. Certain amounts of A and B are mixed in a vessel. As they come to equilibrium

If a catalyst is added to a chemical reaction, the equilibrium yield of a product will be , and the time taken to come to equilibrium will be than before.

The equilibrium constant expression for the reverse of the reaction given below is

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Exam 13: Chemical Equilibrium

Consider the equilibrium system If C is removed, the equilibrium will ____, and if CO is added, the equilibrium will ____.

In a balanced chemical equation, if there is no net change in the total number of moles of gas from the reactant side to the product side, then

If the reaction quotient, Q, is greater than the equilibrium constant, K, then

Which of the following is not true for equilibrium constants?

For an exothermic reaction, an increase in temperature

For the reaction Kc = 1.37. If the concentrations of A and B are equal, what is the value of that concentration?

If the value of Kc for a given reaction at a given temperature is a large number, the energy of the products is likely to be ____ the energy of the reactants because ____.

The equilibrium for a particular chemical reaction is dependent on the

Consider the equilibrium reaction A sample of pure NO2(g) of concentration 0.140 M is allowed to come to equilibrium. It is then found that 57.0 % of the NO2(g) has reacted to form N2O4(g). What is the value of Kc?

Which of the following is false?

Which of the following is true for an equilibrium system?

A particular reaction mixture (Kp = 10) consisting of both gaseous reactants and products is analyzed and is determined to have a value of Q = 15. The pressure of the reaction mixture is then doubled by the addition of argon gas and the reaction is allowed to proceed to equilibrium. At equilibrium

Consider the gas-phase equilibrium A B. Certain amounts of A and B are mixed in a vessel. As they come to equilibrium

If a catalyst is added to a chemical reaction, the equilibrium yield of a product will be ____, and the time taken to come to equilibrium will be ____ than before.

The equilibrium constant expression for the reverse of the reaction given below is

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

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Consider the equilibrium system If C is removed, the equilibrium will , and if CO is added, the equilibrium will .

For the reaction K_c = 1.37. If the concentrations of A and B are equal, what is the value of that concentration?

If the value of K_c for a given reaction at a given temperature is a large number, the energy of the products is likely to be the energy of the reactants because .

Consider the equilibrium reaction A sample of pure NO₂(g) of concentration 0.140 M is allowed to come to equilibrium. It is then found that 57.0 % of the NO₂(g) has reacted to form N₂O₄(g). What is the value of K_c?

A particular reaction mixture (K_p = 10) consisting of both gaseous reactants and products is analyzed and is determined to have a value of Q = 15. The pressure of the reaction mixture is then doubled by the addition of argon gas and the reaction is allowed to proceed to equilibrium. At equilibrium

If a catalyst is added to a chemical reaction, the equilibrium yield of a product will be , and the time taken to come to equilibrium will be than before.