Question 1

Calculate K for the following reaction, provided the concentration versus time graph shown below. 3A   B F1F1F1S1F1F1F10 2C

Accepted Answer

A) 2.0 
B) 10 
C) 22 
D) 31 
E) 44 
A) 2.0 
B) 10 
C) 22 
D) 31 
E) 44

Question 2

A chemical equilibrium may be established by starting a reaction with ________

Accepted Answer

A) reactants only. 
B) products only. 
C) equal quantities of reactants and products. 
D) any quantities of reactants and products. 
E) all of the above. 
A) reactants only. 
B) products only. 
C) equal quantities of reactants and products. 
D) any quantities of reactants and products. 
E) all of the above.

Question 3

The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45.0 at a certain temperature. H2(g) F1F1F1S1F1F1F10 I2(s)   2 HI(g)
Which of the following is true regarding this equilibrium?
I.The reaction is product-favored.
II.The reaction is reactant-favored.
III.Equilibrium lies to the right.
IV.Equilibrium lies to the left.

Accepted Answer

A) I and III 
B) I and IV 
C) II and III 
D) II and IV 
E) None are true, as the concentrations of reactants and products are essentially the same. 
A) I and III 
B) I and IV 
C) II and III 
D) II and IV 
E) None are true, as the concentrations of reactants and products are essentially the same.

Question 4

Chemical equilibrium arises from the ________ of chemical reactions and is reached when the ________ of the forward reaction is equal to the ________ of the reverse reaction.

Accepted Answer

reversibil

Question 5

A chemical equilibrium   A   3B
Has a forward rate constant, sF1F1F1S1F1F1F101 F1F1F1S1F1F1F10 5 M F1F1F1S1F1F1F101sF1F1F1S1F1F1F101, and a reverse rate constant, M F1F1F1S1F1F1F102sF1F1F1S1F1F1F101 F1F1F1S1F1F1F10 0.5 sF1F1F1S1F1F1F101. What is the value of the equilibrium constant for this system?

Accepted Answer

A) 0.1 
B) 0.5 
C) 5.0 
D) 10 
E) 15 
A) 0.1 
B) 0.5 
C) 5.0 
D) 10 
E) 15

Question 6

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown?  A F1F1F1S1F1F1F10 2 B   C
[A] F1F1F1S1F1F1F10 4.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M
[B] F1F1F1S1F1F1F10 2.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 M
[C] F1F1F1S1F1F1F10 9.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M

Accepted Answer

A) 0.22 
B) 9.9 
C) 4.3 F1F1F1S1F1F1F10 105 
D) 2.3 F1F1F1S1F1F1F10 108 
E) 9.5 F1F1F1S1F1F1F10 103 
A) 0.22 
B) 9.9 
C) 4.3 F1F1F1S1F1F1F10 105 
D) 2.3 F1F1F1S1F1F1F10 108 
E) 9.5 F1F1F1S1F1F1F10 103

Question 7

The equilibrium constant for the acid ionization of mercaptoethanol (HSCH2CH2OH ) is 1.91 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010.   HSCH2CH2OH(aq)   HF1F1F1S1F1F1F10(aq) F1F1F1S1F1F1F10 SCH2CH2OHF1F1F1S1F1F1F10(aq)
Which of the following is true regarding this equilibrium?
I.The reaction is product-favored.
II.The reaction is reactant-favored.
III.Equilibrium lies far to the right.
IV.Equilibrium lies far to the left.

Accepted Answer

A) I and III 
B) I and IV 
C) II and III 
D) II and IV 
E) None are true, as the concentrations of reactants and products are comparable. 
A) I and III 
B) I and IV 
C) II and III 
D) II and IV 
E) None are true, as the concentrations of reactants and products are comparable.

Question 8

Which of the following is true for a chemical reaction at equilibrium?

Accepted Answer

A) All reaction has ceased. 
B) The reaction has gone to completion to products. 
C) The amount of reactant(s) remaining is always equal to the amount of product(s) formed. 
D) The rates of the forward and reverse reactions are equal. 
E) The concentrations of products and reactants are still changing. 
A) All reaction has ceased. 
B) The reaction has gone to completion to products. 
C) The amount of reactant(s) remaining is always equal to the amount of product(s) formed. 
D) The rates of the forward and reverse reactions are equal. 
E) The concentrations of products and reactants are still changing.

Question 9

The equilibrium constants for the two reactions are known:
MmF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 4LF1F1F1S1F1F1F10   [ML4]mF1F1F1S1F1F1F104 Ka
HL   HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 LF1F1F1S1F1F1F10 Kb
What must be the value of the equilibrium constant, Koverall, for the following overall reaction?,
MmF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 4HL   [ML4]mF1F1F1S1F1F1F104 F1F1F1S1F1F1F10 4HF1F1F1S1F1F1F10 Koverall

Accepted Answer

Question 10

To solve an equation of the form   for values of x, use ________

Accepted Answer

A) x =   . 
B) ax(x F1F1F1S1F1F1F10 b) = F1F1F1S1F1F1F10c. 
C) x =   . 
D) x =   . 
E) x =   . 
A) x =   . 
B) ax(x F1F1F1S1F1F1F10 b) = F1F1F1S1F1F1F10c. 
C) x =   . 
D) x =   . 
E) x =   .

Question 11

In a reversible reaction A   B at a particular temperature, the rate constant for the reverse reaction is 4 times the rate constant for the forward reaction. What is the value of the equilibrium constant at that temperature?

Accepted Answer

A) Can't tell, need more information. 
B) 0.25 
C) 4 
D) 16 
E) 0.5 
A) Can't tell, need more information. 
B) 0.25 
C) 4 
D) 16 
E) 0.5

Question 12

A decrease in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Accepted Answer

A) Kp F1F1F1S1F1F1F10 Kc. 
B) Kp F1F1F1S1F1F1F10 Kc. 
C) Kp F1F1F1S1F1F1F10 Kc. 
D) Kp F1F1F1S1F1F1F10 Kc F1F1F1S1F1F1F10 (RT )   F1F1F1S1F1F1F10. 
E) KpKc F1F1F1S1F1F1F10 (RT )   F1F1F1S1F1F1F10. 
A) Kp F1F1F1S1F1F1F10 Kc. 
B) Kp F1F1F1S1F1F1F10 Kc. 
C) Kp F1F1F1S1F1F1F10 Kc. 
D) Kp F1F1F1S1F1F1F10 Kc F1F1F1S1F1F1F10 (RT )   F1F1F1S1F1F1F10. 
E) KpKc F1F1F1S1F1F1F10 (RT )   F1F1F1S1F1F1F10.

Question 13

Addition of reactants to a chemical reaction in solution or gas phase at equilibrium results in ________

Accepted Answer

A) an increase in K and a shift in equilibrium to produce more products. 
B) an increase in K and a shift in equilibrium to produce more reactants. 
C) a decrease in K and a shift in equilibrium to produce more products. 
D) a decrease in K and a shift in equilibrium to produce more reactants. 
E) no change in K and a shift in equilibrium to produce more products. 
A) an increase in K and a shift in equilibrium to produce more products. 
B) an increase in K and a shift in equilibrium to produce more reactants. 
C) a decrease in K and a shift in equilibrium to produce more products. 
D) a decrease in K and a shift in equilibrium to produce more reactants. 
E) no change in K and a shift in equilibrium to produce more products.

Question 14

A 10.0 L flask at 500 K is filled with 0.30 mol of hydrogen and 0.30 mol of iodine. They react as indicated below. The equilibrium constant Kc F1F1F1S1F1F1F10 45.0. What are the equilibrium concentrations of the three gases? H2(g) F1F1F1S1F1F1F10 I2(g)   2HI(g)

Accepted Answer

A) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.023 M, [HI] F1F1F1S1F1F1F10 0.046 M 
B) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.0069 M, [HI] F1F1F1S1F1F1F10 0.046 M 
C) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 [HI] F1F1F1S1F1F1F10 0.023 M 
D) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.0069 M, [HI] F1F1F1S1F1F1F10 0.023 M 
E) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.23 M, [HI] F1F1F1S1F1F1F10 0.46 M 
A) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.023 M, [HI] F1F1F1S1F1F1F10 0.046 M 
B) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.0069 M, [HI] F1F1F1S1F1F1F10 0.046 M 
C) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 [HI] F1F1F1S1F1F1F10 0.023 M 
D) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.0069 M, [HI] F1F1F1S1F1F1F10 0.023 M 
E) [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 0.23 M, [HI] F1F1F1S1F1F1F10 0.46 M

Question 15

In a reversible reaction A   B at a particular temperature, the rate constant for the reverse reaction is twice the rate constant for the forward reaction. At equilibrium, how are the concentrations of A and B related?

Accepted Answer

A) Can't tell, need more information. 
B) [A] F1F1F1S1F1F1F10 [B] 
C) [A] F1F1F1S1F1F1F10 2 F1F1F1S1F1F1F10 [B] 
D) [A] F1F1F1S1F1F1F10F1F1F1S1F1F1F10   F1F1F1S1F1F1F10 [B] 
E) [A] F1F1F1S1F1F1F10 4 F1F1F1S1F1F1F10 [B] 
A) Can't tell, need more information. 
B) [A] F1F1F1S1F1F1F10 [B] 
C) [A] F1F1F1S1F1F1F10 2 F1F1F1S1F1F1F10 [B] 
D) [A] F1F1F1S1F1F1F10F1F1F1S1F1F1F10   F1F1F1S1F1F1F10 [B] 
E) [A] F1F1F1S1F1F1F10 4 F1F1F1S1F1F1F10 [B]

Question 16

Which expression corresponds to the equilibrium constant Kc for the reaction written as 2NH3(g) F1F1F1S1F1F1F10 2O2(g)   N2O(g) F1F1F1S1F1F1F10 3H2O2(g)

Accepted Answer

A)    
B)    
C)    
D) [N2O][H2O2]3 
E)    
A)    
B)    
C)    
D) [N2O][H2O2]3 
E)

Question 17

Given the following reactions and associated equilibrium constants     2NO(g) K1 F1F1F1S1F1F1F10 1.70 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1013     NO2(g)
K2 F1F1F1S1F1F1F10 6.83 F1F1F1S1F1F1F10 106
What is the equilibrium constant for the following reaction?
2N2O(g) F1F1F1S1F1F1F10 3O2(g)   4NO2(g) Knew F1F1F1S1F1F1F10 ?

Accepted Answer

A) 1.59 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
B) 9.29 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1018 
C) 40.3 
D) 62.9 
E) 1.08 F1F1F1S1F1F1F10 1017 
A) 1.59 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
B) 9.29 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1018 
C) 40.3 
D) 62.9 
E) 1.08 F1F1F1S1F1F1F10 1017

Question 18

Calculate K for the following reaction, provided the concentration versus time graph shown below.
 2A   2B F1F1F1S1F1F1F10 3C

Accepted Answer

Question 19

Which one of the following is the equilibrium expression, KP, for the reaction that produces lime, CaO, from limestone, CaCO3? CaCO3(s)   CaO(s) F1F1F1S1F1F1F10 CO2(g)

Accepted Answer

A)    
B)    
C)    
D) [CaO][CO2] 
E)    
A)    
B)    
C)    
D) [CaO][CO2] 
E)

Question 20

Given the reaction below, which of the following would cause an increase in the concentration of products? 4NH3(g) F1F1F1S1F1F1F10 3O2(g)   2N2(g) F1F1F1S1F1F1F10 6H2O(g)
I. addition of water
II. removal of ammonia
III. decrease of the volume of the container
IV. addition of oxygen

Accepted Answer

A) I only 
B) II only 
C) IV only 
D) II and III 
E) III and IV 
A) I only 
B) II only 
C) IV only 
D) II and III 
E) III and IV

Calculate K for the following reaction, provided the concentration versus time graph shown below. 3A B  2C

A chemical equilibrium may be established by starting a reaction with ________

Chemical equilibrium arises from the of chemical reactions and is reached when the of the forward reaction is equal to the of the reverse reaction.

A chemical equilibrium A 3B Has a forward rate constant, s^¹  5 M ^¹s^¹, and a reverse rate constant, M ^²s^¹  0.5 s^¹. What is the value of the equilibrium constant for this system?

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown? A  2B C [A]  4.5  10^⁵M [B]  2.2  10^²M [C]  9.4  10^³M

Which of the following is true for a chemical reaction at equilibrium?

The equilibrium constants for the two reactions are known: M^m^  4L^ [ML₄]^m^⁴ K_a HL H^  L^ K_b What must be the value of the equilibrium constant, K_overall, for the following overall reaction?, M^m^  4HL [ML₄]^m^⁴  4H^ K_overall

To solve an equation of the form for values of x, use ________

In a reversible reaction A B at a particular temperature, the rate constant for the reverse reaction is 4 times the rate constant for the forward reaction. What is the value of the equilibrium constant at that temperature?

A decrease in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Addition of reactants to a chemical reaction in solution or gas phase at equilibrium results in ________

A 10.0 L flask at 500 K is filled with 0.30 mol of hydrogen and 0.30 mol of iodine. They react as indicated below. The equilibrium constant K_c  45.0. What are the equilibrium concentrations of the three gases? H₂(g)  I₂(g) 2HI(g)

In a reversible reaction A B at a particular temperature, the rate constant for the reverse reaction is twice the rate constant for the forward reaction. At equilibrium, how are the concentrations of A and B related?

Which expression corresponds to the equilibrium constant K_c for the reaction written as 2NH₃(g)  2O₂(g) N₂O(g)  3H₂O₂(g)

Given the following reactions and associated equilibrium constants 2NO(g) K₁ 1.70  10^¹³ NO₂(g) K₂ 6.83  10⁶ What is the equilibrium constant for the following reaction? 2N₂O(g)  3O₂(g) 4NO₂(g) K_new ?

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B  3C

Which one of the following is the equilibrium expression, K_P, for the reaction that produces lime, CaO, from limestone, CaCO₃? CaCO₃(s) CaO(s)  CO₂(g)

Given the reaction below, which of the following would cause an increase in the concentration of products? 4NH₃(g)  3O₂(g) 2N₂(g)  6H₂O(g) I. addition of water II. removal of ammonia III. decrease of the volume of the container IV. addition of oxygen

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

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Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

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Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

Calculate K for the following reaction, provided the concentration versus time graph shown below. 3A B  2C

A chemical equilibrium may be established by starting a reaction with ________

Chemical equilibrium arises from the ________ of chemical reactions and is reached when the ________ of the forward reaction is equal to the ________ of the reverse reaction.

A chemical equilibrium A 3B Has a forward rate constant, s1  5 M 1s1, and a reverse rate constant, M 2s1  0.5 s1. What is the value of the equilibrium constant for this system?

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown? A  2 B C [A]  4.5  105 M [B]  2.2  102 M [C]  9.4  103 M

Which of the following is true for a chemical reaction at equilibrium?

The equilibrium constants for the two reactions are known: Mm  4L [ML4]m4 Ka HL H  L Kb What must be the value of the equilibrium constant, Koverall, for the following overall reaction?, Mm  4HL [ML4]m4  4H Koverall

To solve an equation of the form for values of x, use ________

In a reversible reaction A B at a particular temperature, the rate constant for the reverse reaction is 4 times the rate constant for the forward reaction. What is the value of the equilibrium constant at that temperature?

A decrease in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Addition of reactants to a chemical reaction in solution or gas phase at equilibrium results in ________

A 10.0 L flask at 500 K is filled with 0.30 mol of hydrogen and 0.30 mol of iodine. They react as indicated below. The equilibrium constant Kc  45.0. What are the equilibrium concentrations of the three gases? H2(g)  I2(g) 2HI(g)

In a reversible reaction A B at a particular temperature, the rate constant for the reverse reaction is twice the rate constant for the forward reaction. At equilibrium, how are the concentrations of A and B related?

Which expression corresponds to the equilibrium constant Kc for the reaction written as 2NH3(g)  2O2(g) N2O(g)  3H2O2(g)

Given the following reactions and associated equilibrium constants 2NO(g) K1  1.70  1013 NO2(g) K2  6.83  106 What is the equilibrium constant for the following reaction? 2N2O(g)  3O2(g) 4NO2(g) Knew  ?

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B  3C

Which one of the following is the equilibrium expression, KP, for the reaction that produces lime, CaO, from limestone, CaCO3? CaCO3(s) CaO(s)  CO2(g)

Given the reaction below, which of the following would cause an increase in the concentration of products? 4NH3(g)  3O2(g) 2N2(g)  6H2O(g) I. addition of water II. removal of ammonia III. decrease of the volume of the container IV. addition of oxygen

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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Chemical equilibrium arises from the of chemical reactions and is reached when the of the forward reaction is equal to the of the reverse reaction.

A chemical equilibrium A 3B Has a forward rate constant, s^¹  5 M ^¹s^¹, and a reverse rate constant, M ^²s^¹  0.5 s^¹. What is the value of the equilibrium constant for this system?

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown? A  2B C [A]  4.5  10^⁵M [B]  2.2  10^²M [C]  9.4  10^³M

The equilibrium constants for the two reactions are known: M^m^  4L^ [ML₄]^m^⁴ K_a HL H^  L^ K_b What must be the value of the equilibrium constant, K_overall, for the following overall reaction?, M^m^  4HL [ML₄]^m^⁴  4H^ K_overall

A 10.0 L flask at 500 K is filled with 0.30 mol of hydrogen and 0.30 mol of iodine. They react as indicated below. The equilibrium constant K_c  45.0. What are the equilibrium concentrations of the three gases? H₂(g)  I₂(g) 2HI(g)

Which expression corresponds to the equilibrium constant K_c for the reaction written as 2NH₃(g)  2O₂(g) N₂O(g)  3H₂O₂(g)

Given the following reactions and associated equilibrium constants 2NO(g) K₁ 1.70  10^¹³ NO₂(g) K₂ 6.83  10⁶ What is the equilibrium constant for the following reaction? 2N₂O(g)  3O₂(g) 4NO₂(g) K_new ?

Which one of the following is the equilibrium expression, K_P, for the reaction that produces lime, CaO, from limestone, CaCO₃? CaCO₃(s) CaO(s)  CO₂(g)

Given the reaction below, which of the following would cause an increase in the concentration of products? 4NH₃(g)  3O₂(g) 2N₂(g)  6H₂O(g) I. addition of water II. removal of ammonia III. decrease of the volume of the container IV. addition of oxygen