Question 1

A reaction that can proceed in either the forward or the reverse direction as written is called a __________ reaction.

Accepted Answer

A)  reversible 
B)  miniscule 
C)  microscopic 
D)  solid phase 
E)  favored 
A)  reversible 
B)  miniscule 
C)  microscopic 
D)  solid phase 
E)  favored

Question 2

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen?

Accepted Answer

A)  The equilibrium constant for the binding of CO is greater. 
B)  The equilibrium constant for the binding of oxygen is greater. 
C)  The concentration of carbon monoxide at equilibrium is twice that of oxygen. 
D)  Oxygen and carbon monoxide have the same formula mass. 
E)  Oxygen and carbon monoxide react with hemoglobin in different fashions. 
A)  The equilibrium constant for the binding of CO is greater. 
B)  The equilibrium constant for the binding of oxygen is greater. 
C)  The concentration of carbon monoxide at equilibrium is twice that of oxygen. 
D)  Oxygen and carbon monoxide have the same formula mass. 
E)  Oxygen and carbon monoxide react with hemoglobin in different fashions.

Question 3

What is the correct form for the equilibrium constant expression for this reaction? 
H?(g) + F2(g) ? 2 HF(g)

Accepted Answer

A)  $\frac { [ \mathrm { HF } ] } { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] }$ 
B)  $\frac { [ \mathrm { HF } ] ^ { 2 } } { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] }$ 
C)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { [ \mathrm { HF } ] }$ 
D)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { [ \mathrm { HF } ] ^ { 2 } }$ 
E)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { 2 [ \mathrm { HF } ] }$ 
A)  $\frac { [ \mathrm { HF } ] } { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] }$ 
B)  $\frac { [ \mathrm { HF } ] ^ { 2 } } { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] }$ 
C)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { [ \mathrm { HF } ] }$ 
D)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { [ \mathrm { HF } ] ^ { 2 } }$ 
E)  $\frac { \left[ \mathrm { H } _ { 2 } \right] \left[ \mathrm { F } _ { 2 } \right] } { 2 [ \mathrm { HF } ] }$

Question 4

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is Kc = 2 × 1011. This means that the reaction mixture at equilibrium is likely to consist of

Accepted Answer

A)  mostly starting materials. 
B)  an equal mixture of products and reactants. 
C)  twice as much starting material as product. 
D)  twice as much product as starting material. 
E)  mostly products. 
A)  mostly starting materials. 
B)  an equal mixture of products and reactants. 
C)  twice as much starting material as product. 
D)  twice as much product as starting material. 
E)  mostly products.

Question 5

An example of a stress on an equilibrium is the increase of pressure in a closed system when the pressure of a reactant gas is increased from 1.0 atm to 2.0 atm.

Accepted Answer

A) True 
 B)False

Question 6

In any chemical reaction, the rate of the reaction can be increased by

Accepted Answer

A)  decreasing the temperature. 
B)  changing the size of the container. 
C)  adding water to the reaction. 
D)  adding product molecules to the reaction mixture. 
E)  increasing the concentrations of the reactants. 
A)  decreasing the temperature. 
B)  changing the size of the container. 
C)  adding water to the reaction. 
D)  adding product molecules to the reaction mixture. 
E)  increasing the concentrations of the reactants.

Question 7

An equilibrium constant Kc = 1 × 10-3 for a reaction indicates that the reaction favors product formation.

Accepted Answer

A) True 
 B)False

Question 8

The activation energy of a chemical reaction is the energy that

Accepted Answer

A)  must be removed from the mixture. 
B)  must be released from the mixture. 
C)  initiates the reaction. 
D)  activates the catalyst. 
E)  is the difference in the energies of the starting materials and products. 
A)  must be removed from the mixture. 
B)  must be released from the mixture. 
C)  initiates the reaction. 
D)  activates the catalyst. 
E)  is the difference in the energies of the starting materials and products.

Question 9

In a catalytic converter in an automobile, the reaction of carbon monoxide with oxygen produces __________.

Accepted Answer

A)  carbon dioxide 
B)  carbon and more oxygen 
C)  water 
D)  methane 
E)  nitrogen oxide 
A)  carbon dioxide 
B)  carbon and more oxygen 
C)  water 
D)  methane 
E)  nitrogen oxide

Question 10

What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? The equation is: 
2H?(g) + O?(g) ? H?O(g)

Accepted Answer

A)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 2 } }$ 
B)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] }$ 
C)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } ^ { 2 } \right] }$ 
D)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ 2 \mathrm { H } _ { 2 } \right] }$ 
E)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } ^ { 2 } \right] }$ 
A)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 2 } }$ 
B)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] }$ 
C)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } ^ { 2 } \right] }$ 
D)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { O } _ { 2 } \right] \left[ 2 \mathrm { H } _ { 2 } \right] }$ 
E)  Kc = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } } { \left[ \mathrm { O } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } ^ { 2 } \right] }$

Question 11

The rule or principle that describes the effect of changing reaction conditions on an equilibrium is known as __________ principle.

Accepted Answer

The answer of The rule or principle that describes the...

Question 12

One metal that is used as a catalyst in a catalytic converter in an automobile is __________.

Accepted Answer

A)  carbon 
B)  iron 
C)  copper 
D)  platinum 
E)  plutonium 
A)  carbon 
B)  iron 
C)  copper 
D)  platinum 
E)  plutonium

Question 13

PCl5 (g) ⇌ PCl3 (g)+ Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present will

Accepted Answer

A)  decrease. 
B)  increase. 
C)  double. 
D)  stay the same. 
E)  triple. 
A)  decrease. 
B)  increase. 
C)  double. 
D)  stay the same. 
E)  triple.

Question 14

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

Accepted Answer

A)  The concentration of products exceeds the concentration of reactants. 
B)  The concentrations of reactants and products are equal. 
C)  The reactants are solids. 
D)  The concentration of reactants exceeds the concentration of products. 
E)  The products are solids. 
A)  The concentration of products exceeds the concentration of reactants. 
B)  The concentrations of reactants and products are equal. 
C)  The reactants are solids. 
D)  The concentration of reactants exceeds the concentration of products. 
E)  The products are solids.

Question 15

The rate of any chemical reaction can be determined by observing

Accepted Answer

A)  the amount of product formed in a unit of time. 
B)  the ratio of product concentration to reactant concentration. 
C)  the percent composition of the final product. 
D)  the theoretical yield of the reaction. 
E)  the number of chemical bonds broken and remade. 
A)  the amount of product formed in a unit of time. 
B)  the ratio of product concentration to reactant concentration. 
C)  the percent composition of the final product. 
D)  the theoretical yield of the reaction. 
E)  the number of chemical bonds broken and remade.

Question 16

The equilibrium constant for the formation of ammonia from nitrogen and hydrogen is 1.6 × 102. What is the form of the equilibrium constant?

Accepted Answer

A)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
B)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] } { \left[ \mathrm { N } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
C)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] }$ 
D)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ 3 \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
E)  $\frac { \left[ 2 \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
A)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
B)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] } { \left[ \mathrm { N } _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
C)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] }$ 
D)  $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ 3 \mathrm { H } _ { 2 } \right] ^ { 3 } }$ 
E)  $\frac { \left[ 2 \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$

Question 17

The rate of a chemical reaction depends on temperature.

Accepted Answer

A) True 
 B)False

Question 18

The equilibrium constant for a reaction does not change with temperature.

Accepted Answer

A) True 
 B)False

Question 19

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of __________ in a clinical setting.

Accepted Answer

A)  the ideal gas law 
B)  Le Chatelier's principle 
C)  Henry's law 
D)  conservation of mass 
E)  a precipitation reaction 
A)  the ideal gas law 
B)  Le Chatelier's principle 
C)  Henry's law 
D)  conservation of mass 
E)  a precipitation reaction

Question 20

The equilibrium between hemoglobin and oxyhemoglobin in the blood can be represented by the following reaction. Write the form of the equilibrium constant expression.
Hb + O₂ ⇌ HbO₂

Accepted Answer

The answer of The equilibrium between hemoglobin and oxyhemoglobin in...

Exam 9: Reaction Rates and Chemical Equilibrium

A reaction that can proceed in either the forward or the reverse direction as written is called a __________ reaction.

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen?

What is the correct form for the equilibrium constant expression for this reaction? H?(g) + F2(g) ? 2 HF(g)

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is Kc = 2 × 1011. This means that the reaction mixture at equilibrium is likely to consist of

An example of a stress on an equilibrium is the increase of pressure in a closed system when the pressure of a reactant gas is increased from 1.0 atm to 2.0 atm.

In any chemical reaction, the rate of the reaction can be increased by

An equilibrium constant Kc = 1 × 10-3 for a reaction indicates that the reaction favors product formation.

The activation energy of a chemical reaction is the energy that

In a catalytic converter in an automobile, the reaction of carbon monoxide with oxygen produces __________.

What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? The equation is: 2H?(g) + O?(g) ? H?O(g)

The rule or principle that describes the effect of changing reaction conditions on an equilibrium is known as __________ principle.

One metal that is used as a catalyst in a catalytic converter in an automobile is __________.

PCl5 (g) ⇌ PCl3 (g)+ Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present will

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

The rate of any chemical reaction can be determined by observing

The equilibrium constant for the formation of ammonia from nitrogen and hydrogen is 1.6 × 102. What is the form of the equilibrium constant?

The rate of a chemical reaction depends on temperature.

The equilibrium constant for a reaction does not change with temperature.

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of __________ in a clinical setting.

The equilibrium between hemoglobin and oxyhemoglobin in the blood can be represented by the following reaction. Write the form of the equilibrium constant expression. Hb + O₂ ⇌ HbO₂

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What is the correct form for the equilibrium constant expression for this reaction? H?(g) + F₂(g) ? 2 HF(g)

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K_c = 2 × 10¹¹. This means that the reaction mixture at equilibrium is likely to consist of

An equilibrium constant K_c = 1 × 10^-3 for a reaction indicates that the reaction favors product formation.

PCl₅ (g) ⇌ PCl₃ (g)+ Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl₅ present will

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10^-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

The equilibrium constant for the formation of ammonia from nitrogen and hydrogen is 1.6 × 10². What is the form of the equilibrium constant?