Question 1

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 2

Which compound below is the most soluble in water based on its   value?

Accepted Answer

A) CuS,   = 1.27   
B) PbS,   = 9.04   
C) AgCl,   = 1.77   
D) AgI,   = 8.51   
E) not enough information 
A) CuS,   = 1.27   
B) PbS,   = 9.04   
C) AgCl,   = 1.77   
D) AgI,   = 8.51   
E) not enough information

Question 3

Which of the following changes will increase reaction rate? 
1.An increase in the concentration of reactants
2.An increase in temperature
3.Higher-energy collisions between reacting molecules

Accepted Answer

A) 1 and 2 only 
B) 1 and 3 only 
C) 2 and 3 only 
D) All of 1,2,and 3 
E) Neither 1,2,or 3 
A) 1 and 2 only 
B) 1 and 3 only 
C) 2 and 3 only 
D) All of 1,2,and 3 
E) Neither 1,2,or 3

Question 4

Which of the following equilibrium systems will shift to the right (towards products)when pressure is increased.

Accepted Answer

A) 2 PbS (s)+ 3O2 (g)⇌ 2PbO (s)+ 2 SO2 (g) 
B) PCl5 (g)⇌ PCl3 (g)+ Cl2 (g) 
C) H2 (g)+ CO2 (g)⇌   O (g)+ CO (g) 
D) all of these 
E) none of these 
A) 2 PbS (s)+ 3O2 (g)⇌ 2PbO (s)+ 2 SO2 (g) 
B) PCl5 (g)⇌ PCl3 (g)+ Cl2 (g) 
C) H2 (g)+ CO2 (g)⇌   O (g)+ CO (g) 
D) all of these 
E) none of these

Question 5

A compound with a relatively small   value indicates that the compound is only partially soluble.

Accepted Answer

A) True 
 B)False

Question 6

Which of the following is TRUE for a system that is in dynamic equilibrium?

Accepted Answer

A) The forward reaction goes to 100% completion. 
B) The reaction rate of the forward reaction approaches zero. 
C) The concentration of products is equal to the concentration of the reactants. 
D) Both the forward and reverse reactions come to a halt. 
E) none of the above 
A) The forward reaction goes to 100% completion. 
B) The reaction rate of the forward reaction approaches zero. 
C) The concentration of products is equal to the concentration of the reactants. 
D) Both the forward and reverse reactions come to a halt. 
E) none of the above

Question 7

If Keq = 2 for the reaction X ⇌ Y,then the Keq for Y ⇌ X will be 1/2 (or 0.5).

Accepted Answer

A) True 
 B)False

Question 8

The chemical equation that would generate the equilibrium expression  is ________.(Assume all substances are gases in this reaction.)

Accepted Answer

A) C + 2B ⇌ 3A 
B) 3A ⇌ 2B + C 
C) A ⇌ B + C 
D) 1/2 B + C ⇌ 1/3 A 
E) none of the above 
A) C + 2B ⇌ 3A 
B) 3A ⇌ 2B + C 
C) A ⇌ B + C 
D) 1/2 B + C ⇌ 1/3 A 
E) none of the above

Question 9

For the reaction H2 (g)+ Cl2 (g)⇌ 2 HCl (g),what happens to the equilibrium position if the pressure increases?

Accepted Answer

A) shifts to the right 
B) shifts to the left 
C) does nothing 
D) doubles 
E) none of the above 
A) shifts to the right 
B) shifts to the left 
C) does nothing 
D) doubles 
E) none of the above

Question 10

For the reaction  ,what happens to the equilibrium position if the amount of silver ion is halved?

Accepted Answer

A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves 
A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves

Question 11

Reaction rates generally increase as a reaction proceeds.

Accepted Answer

A) True 
 B)False

Question 12

The equilibrium constant,   ,for an equilibrium reaction will always be the same (at a given temperature)regardless of what the initial concentrations of reactants and products were.

Accepted Answer

A) True 
 B)False

Question 13

The rate of a reaction increases with increasing concentrations of reactants because you have more collisions occurring in a given time period.

Accepted Answer

A) True 
 B)False

Question 14

For the reaction   ,the equilibrium concentrations are as follows:   ,   ,   .The equilibrium constant is:

Accepted Answer

A) 7.53 ×   
B) 1.19 ×   
C) 8.43   
D) 1.33 ×   
E) none of the above 
A) 7.53 ×   
B) 1.19 ×   
C) 8.43   
D) 1.33 ×   
E) none of the above

Question 15

A chemical equilibrium exists when:

Accepted Answer

A) reactants are completely changed to products. 
B) there are equal amounts of reactants and products. 
C) the rate at which reactants form products becomes zero. 
D) the sum of reactant and product concentrations equals one mole. 
E) the rate at which reactants form products is the same as the rate at which products form reactants. 
A) reactants are completely changed to products. 
B) there are equal amounts of reactants and products. 
C) the rate at which reactants form products becomes zero. 
D) the sum of reactant and product concentrations equals one mole. 
E) the rate at which reactants form products is the same as the rate at which products form reactants.

Question 16

The rate of a chemical reaction always remains the same from start to finish.

Accepted Answer

A) True 
 B)False

Question 17

Calculate the concentration of NO2 in an equilibrium mixture given that the concentration of   and   for the reaction:

Accepted Answer

A) 0.0663 M 
B) 0.00440 M 
C) 227.3 M 
D) 15.1 M 
E) none of the above 
A) 0.0663 M 
B) 0.00440 M 
C) 227.3 M 
D) 15.1 M 
E) none of the above

Question 18

Identify the equation for which

Accepted Answer

A)   
B)   
C)   
D)   
E) none of the above 
A)   
B)   
C)   
D)   
E) none of the above

Question 19

Collisions between reactant molecules do not always lead to the formation of product molecules.

Accepted Answer

A) True 
 B)False

Question 20

For the reaction 2A + B ⇌ 2C + 3D,the equilibrium expression is:

Accepted Answer

A)    =   
B)    =   
C)    =   
D)    =   
E) none of the above 
A)    =   
B)    =   
C)    =   
D)    =   
E) none of the above

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.

Which compound below is the most soluble in water based on its value?

Which of the following changes will increase reaction rate? 1.An increase in the concentration of reactants 2.An increase in temperature 3.Higher-energy collisions between reacting molecules

Which of the following equilibrium systems will shift to the right (towards products)when pressure is increased.

A compound with a relatively small value indicates that the compound is only partially soluble.

Which of the following is TRUE for a system that is in dynamic equilibrium?

If K_eq = 2 for the reaction X ⇌ Y,then the K_eq for Y ⇌ X will be 1/2 (or 0.5).

The chemical equation that would generate the equilibrium expression is ________.(Assume all substances are gases in this reaction.)

For the reaction H₂ (g)+ Cl₂ (g)⇌ 2 HCl (g),what happens to the equilibrium position if the pressure increases?

For the reaction ,what happens to the equilibrium position if the amount of silver ion is halved?

Reaction rates generally increase as a reaction proceeds.

The equilibrium constant, ,for an equilibrium reaction will always be the same (at a given temperature)regardless of what the initial concentrations of reactants and products were.

The rate of a reaction increases with increasing concentrations of reactants because you have more collisions occurring in a given time period.

For the reaction ,the equilibrium concentrations are as follows: , , .The equilibrium constant is:

A chemical equilibrium exists when:

The rate of a chemical reaction always remains the same from start to finish.

Calculate the concentration of NO₂ in an equilibrium mixture given that the concentration of and for the reaction:

Identify the equation for which

Collisions between reactant molecules do not always lead to the formation of product molecules.

For the reaction 2A + B ⇌ 2C + 3D,the equilibrium expression is:

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Exam 15: Chemical Equilibrium

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.

Which compound below is the most soluble in water based on its value?

Which of the following changes will increase reaction rate? 1.An increase in the concentration of reactants 2.An increase in temperature 3.Higher-energy collisions between reacting molecules

Which of the following equilibrium systems will shift to the right (towards products)when pressure is increased.

A compound with a relatively small value indicates that the compound is only partially soluble.

Which of the following is TRUE for a system that is in dynamic equilibrium?

If Keq = 2 for the reaction X ⇌ Y,then the Keq for Y ⇌ X will be 1/2 (or 0.5).

The chemical equation that would generate the equilibrium expression is ________.(Assume all substances are gases in this reaction.)

For the reaction H2 (g)+ Cl2 (g)⇌ 2 HCl (g),what happens to the equilibrium position if the pressure increases?

For the reaction ,what happens to the equilibrium position if the amount of silver ion is halved?

Reaction rates generally increase as a reaction proceeds.

The equilibrium constant, ,for an equilibrium reaction will always be the same (at a given temperature)regardless of what the initial concentrations of reactants and products were.

The rate of a reaction increases with increasing concentrations of reactants because you have more collisions occurring in a given time period.

For the reaction ,the equilibrium concentrations are as follows: , , .The equilibrium constant is:

A chemical equilibrium exists when:

The rate of a chemical reaction always remains the same from start to finish.

Calculate the concentration of NO2 in an equilibrium mixture given that the concentration of and for the reaction:

Identify the equation for which

Collisions between reactant molecules do not always lead to the formation of product molecules.

For the reaction 2A + B ⇌ 2C + 3D,the equilibrium expression is:

The Chemical World

Measurement and Problem Solving

Matter and Energy

Atoms and Elements

Molecules and Compounds

Chemical Composition

Chemical Reactions

Quantities in Chemical Reactions

Electrons in Atoms and the Periodic Table

Chemical Bonding

Gases

Liquids, solids, and Intermolecular Forces

Solutions

Acids and Bases

Oxidation and Reduction

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

If K_eq = 2 for the reaction X ⇌ Y,then the K_eq for Y ⇌ X will be 1/2 (or 0.5).

For the reaction H₂ (g)+ Cl₂ (g)⇌ 2 HCl (g),what happens to the equilibrium position if the pressure increases?

Calculate the concentration of NO₂ in an equilibrium mixture given that the concentration of and for the reaction: