Question 1

What will happen to a system at equilibrium when that equilibrium is disturbed?

Accepted Answer

It will shift to counteract the disturbance and reestablish an equilibrium.

Question 2

In the following reaction: HC2H3O2 ⇌ H+ + C2H3O2-, if [HC2H3O2] = 0.28 M and the pH = 5.0, what is K?

Accepted Answer

A) 3.57 × 10-10 
B) 1.00 × 10-4 
C) 1.00 × 10-10 
D) 3.57 × 10-4 
A) 3.57 × 10-10 
B) 1.00 × 10-4 
C) 1.00 × 10-10 
D) 3.57 × 10-4 A

Question 3

What does it mean when the value of an equilibrium constant for a reaction is at or close to 1?

Accepted Answer

A) The value of the product concentration term divided by the reactant concentration term is at or close to 1. 
B) The value of the product concentration term must be at or close to 1. 
C) The value of the reactant concentration term or the product concentration term must be at or close to 1. 
D) The value of the product concentration term divided by the reactant concentration term is at or close to 1 because the value of each concentration term is at or close to 1. 
A) The value of the product concentration term divided by the reactant concentration term is at or close to 1. 
B) The value of the product concentration term must be at or close to 1. 
C) The value of the reactant concentration term or the product concentration term must be at or close to 1. 
D) The value of the product concentration term divided by the reactant concentration term is at or close to 1 because the value of each concentration term is at or close to 1. A

Question 4

A catalyst added to a system going to equilibrium does what?

Accepted Answer

A) Raises the activation energy of the reverse reaction 
B) Lowers the activation energy for the forward reaction 
C) Increases each reaction's rate, allowing equilibrium to be reached faster 
D) Nothing 
A) Raises the activation energy of the reverse reaction 
B) Lowers the activation energy for the forward reaction 
C) Increases each reaction's rate, allowing equilibrium to be reached faster 
D) Nothing

Question 5

During or immediately after carbon monoxide poisoning, what should be done to shift the equilibrium to the production of oxyhemoglobin?

Accepted Answer

A) Expose the affected person to oxygen. 
B) Limit the affected person's exposure to oxygen. 
C) Expose the affected person to a progressively decreasing CO/O2 mixture. 
D) Expose the affected person to a low-pressure atmosphere. 
A) Expose the affected person to oxygen. 
B) Limit the affected person's exposure to oxygen. 
C) Expose the affected person to a progressively decreasing CO/O2 mixture. 
D) Expose the affected person to a low-pressure atmosphere.

Question 6

What else, besides energy of activation, influences both equilibrium reactions?

Accepted Answer

Frequency of collisi

Question 7

In the following reaction: HBr ⇌ H+ + Br- , what is the pH value if [HBr] = 0.120 M and K = 1 × 10-8?

Accepted Answer

A) 3.46 
B) 4.46 
C) 0.45 
D) 1.20 
A) 3.46 
B) 4.46 
C) 0.45 
D) 1.20

Question 8

How does the energy of activation restrict an equilibrium reaction?

Accepted Answer

A) It limits the molecules that will have enough energy to react. 
B) It cools the reaction by draining it of energy. 
C) It blocks the forward reaction with the formation of products. 
D) It slows both forward and reverse reactions. 
A) It limits the molecules that will have enough energy to react. 
B) It cools the reaction by draining it of energy. 
C) It blocks the forward reaction with the formation of products. 
D) It slows both forward and reverse reactions.

Question 9

What is the formula of arsenopyrite?

Accepted Answer

A) FeAsS 
B) FeS 
C) AsS 
D) FeAs 
A) FeAsS 
B) FeS 
C) AsS 
D) FeAs

Question 10

What controls both the forward and reverse reactions of an equilibrium?

Accepted Answer

A) Activation energy barrier 
B) Restrictions of collision theory 
C) Both of the above 
D) None of the above 
A) Activation energy barrier 
B) Restrictions of collision theory 
C) Both of the above 
D) None of the above

Question 11

Why is sodium chloride, which is far more soluble in water than arsenic oxide, not considered a poison?

Accepted Answer

A) It is not soluble enough to be a poison. 
B) It passes through the human body too quickly. 
C) Its LD50 is considerably higher than the amount normally consumed, either in water or in food. 
D) None of the above; sodium chloride is considered a poison. 
A) It is not soluble enough to be a poison. 
B) It passes through the human body too quickly. 
C) Its LD50 is considerably higher than the amount normally consumed, either in water or in food. 
D) None of the above; sodium chloride is considered a poison.

Question 12

In the reaction As2S3(s) ⇌ 2As3+(aq) + 3S2-(aq), how could more arsenic be brought into solution?

Accepted Answer

More react

Question 13

In an equilibrium whose reaction is expressed HAc ⇌ H+ + Ac- , how can K equal a number greater than 1000 if the product concentrations are never greater than 0.2 M each?

Accepted Answer

A) The product concentrations must be halved. 
B) The reactant concentration must be as small as 4.0 × 10-5. 
C) The reactant concentrations must be made as large as 5.0 × 105. 
D) The product concentrations must be very close to zero. 
A) The product concentrations must be halved. 
B) The reactant concentration must be as small as 4.0 × 10-5. 
C) The reactant concentrations must be made as large as 5.0 × 105. 
D) The product concentrations must be very close to zero.

Question 14

In the reaction: N2 + 3 H2 ⇌ 2 NH3, the equilibrium constant is very small, yet ammonia (NH3) is readily produced. What conditions might be applied to make this happen?

Accepted Answer

A) A catalyst is added. 
B) Product is removed as soon as it is formed. 
C) All of the above. 
D) None of the above. 
A) A catalyst is added. 
B) Product is removed as soon as it is formed. 
C) All of the above. 
D) None of the above.

Question 15

How does arsenic dissolve and thus get into ground water?

Accepted Answer

A) From plant sources near the ground water 
B) From an equilibrium with soluble arsenic ions 
C) From an equilibrium with insoluble arsenic ions 
D) From soluble plant matter near the ground water 
A) From plant sources near the ground water 
B) From an equilibrium with soluble arsenic ions 
C) From an equilibrium with insoluble arsenic ions 
D) From soluble plant matter near the ground water

Question 16

If a system in equilibrium begins shifting in concentration to the product's side, what may have caused the shift?

Accepted Answer

A) A catalyst was added to the system. 
B) Products were added to the system. 
C) Reactants were removed from the system. 
D) Reactants were added to the system. 
A) A catalyst was added to the system. 
B) Products were added to the system. 
C) Reactants were removed from the system. 
D) Reactants were added to the system.

Question 17

What is the [H+] in the following reaction: HA ⇌ H+ + A- , when [HA] = 0.050 M and K = 0.28?

Accepted Answer

A) 0.118 M 
B) 0.014 M 
C) 5.60 M 
D) 2.36 M 
A) 0.118 M 
B) 0.014 M 
C) 5.60 M 
D) 2.36 M

Question 18

What is K the symbol for in an equilibrium?

Accepted Answer

A) The equilibrium constant 
B) The product concentration 
C) The reactant concentration 
D) The equilibrium percentage 
A) The equilibrium constant 
B) The product concentration 
C) The reactant concentration 
D) The equilibrium percentage

Question 19

What is the pH in the following reaction: HI ⇌ H+ + I- , if the [HI] = 0.250 M and K = 1 × 10-6?

Accepted Answer

A) 3.30 
B) 5.00 
C) 2.50 
D) 0.25 
A) 3.30 
B) 5.00 
C) 2.50 
D) 0.25

Question 20

To what does a body metabolize ethylene glycol?

Accepted Answer

Oxalic acid (which t

What will happen to a system at equilibrium when that equilibrium is disturbed?

In the following reaction: HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^-, if [HC₂H₃O₂] = 0.28 M and the pH = 5.0, what is K?

What does it mean when the value of an equilibrium constant for a reaction is at or close to 1?

A catalyst added to a system going to equilibrium does what?

During or immediately after carbon monoxide poisoning, what should be done to shift the equilibrium to the production of oxyhemoglobin?

What else, besides energy of activation, influences both equilibrium reactions?

In the following reaction: HBr ⇌ H⁺ + Br^- , what is the pH value if [HBr] = 0.120 M and K = 1 × 10^-8?

How does the energy of activation restrict an equilibrium reaction?

What is the formula of arsenopyrite?

What controls both the forward and reverse reactions of an equilibrium?

Why is sodium chloride, which is far more soluble in water than arsenic oxide, not considered a poison?

In the reaction As₂S_3(s) ⇌ 2As³⁺_(aq) + 3S^2-_(aq), how could more arsenic be brought into solution?

In an equilibrium whose reaction is expressed HAc ⇌ H⁺ + Ac^- , how can K equal a number greater than 1000 if the product concentrations are never greater than 0.2 M each?

In the reaction: N₂ + 3 H₂ ⇌ 2 NH₃, the equilibrium constant is very small, yet ammonia (NH₃) is readily produced. What conditions might be applied to make this happen?

How does arsenic dissolve and thus get into ground water?

If a system in equilibrium begins shifting in concentration to the product's side, what may have caused the shift?

What is the [H⁺] in the following reaction: HA ⇌ H⁺ + A^- , when [HA] = 0.050 M and K = 0.28?

What is K the symbol for in an equilibrium?

What is the pH in the following reaction: HI ⇌ H⁺ + I^- , if the [HI] = 0.250 M and K = 1 × 10^-6?

To what does a body metabolize ethylene glycol?

Understanding Our World With Chemistry

Matter: Properties, Changes and Measurements

Understanding Atoms

Bonding and Reactions

Chemistry of Bonding: Structure and Function of Drug Molecules

Aqueous Solutions: Part I

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Chemistry of Fire and Heat

Chemistry of Explosions

Applications of Chemical Kinetics

Nuclear Chemistry: Energy, Medicine, Weapons, and Terrorism

Introduction to Biochemistry

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Exam 13: Chemical Equilibrium

What will happen to a system at equilibrium when that equilibrium is disturbed?

In the following reaction: HC2H3O2 ⇌ H+ + C2H3O2-, if [HC2H3O2] = 0.28 M and the pH = 5.0, what is K?

What does it mean when the value of an equilibrium constant for a reaction is at or close to 1?

A catalyst added to a system going to equilibrium does what?

During or immediately after carbon monoxide poisoning, what should be done to shift the equilibrium to the production of oxyhemoglobin?

What else, besides energy of activation, influences both equilibrium reactions?

In the following reaction: HBr ⇌ H+ + Br- , what is the pH value if [HBr] = 0.120 M and K = 1 × 10-8?

How does the energy of activation restrict an equilibrium reaction?

What is the formula of arsenopyrite?

What controls both the forward and reverse reactions of an equilibrium?

Why is sodium chloride, which is far more soluble in water than arsenic oxide, not considered a poison?

In the reaction As2S3(s) ⇌ 2As3+(aq) + 3S2-(aq), how could more arsenic be brought into solution?

In an equilibrium whose reaction is expressed HAc ⇌ H+ + Ac- , how can K equal a number greater than 1000 if the product concentrations are never greater than 0.2 M each?

In the reaction: N2 + 3 H2 ⇌ 2 NH3, the equilibrium constant is very small, yet ammonia (NH3) is readily produced. What conditions might be applied to make this happen?

How does arsenic dissolve and thus get into ground water?

If a system in equilibrium begins shifting in concentration to the product's side, what may have caused the shift?

What is the [H+] in the following reaction: HA ⇌ H+ + A- , when [HA] = 0.050 M and K = 0.28?

What is K the symbol for in an equilibrium?

What is the pH in the following reaction: HI ⇌ H+ + I- , if the [HI] = 0.250 M and K = 1 × 10-6?

To what does a body metabolize ethylene glycol?

Understanding Our World With Chemistry

Matter: Properties, Changes and Measurements

Understanding Atoms

Bonding and Reactions

Chemistry of Bonding: Structure and Function of Drug Molecules

Aqueous Solutions: Part I

Aqueous Solutions: Part II

Organic Chemistry and Polymers

Chemistry of Fire and Heat

Chemistry of Explosions

Applications of Chemical Kinetics

Nuclear Chemistry: Energy, Medicine, Weapons, and Terrorism

Introduction to Biochemistry

Filters

In the following reaction: HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^-, if [HC₂H₃O₂] = 0.28 M and the pH = 5.0, what is K?

In the following reaction: HBr ⇌ H⁺ + Br^- , what is the pH value if [HBr] = 0.120 M and K = 1 × 10^-8?

In the reaction As₂S_3(s) ⇌ 2As³⁺_(aq) + 3S^2-_(aq), how could more arsenic be brought into solution?

In an equilibrium whose reaction is expressed HAc ⇌ H⁺ + Ac^- , how can K equal a number greater than 1000 if the product concentrations are never greater than 0.2 M each?

In the reaction: N₂ + 3 H₂ ⇌ 2 NH₃, the equilibrium constant is very small, yet ammonia (NH₃) is readily produced. What conditions might be applied to make this happen?

What is the [H⁺] in the following reaction: HA ⇌ H⁺ + A^- , when [HA] = 0.050 M and K = 0.28?

What is the pH in the following reaction: HI ⇌ H⁺ + I^- , if the [HI] = 0.250 M and K = 1 × 10^-6?