Question 1

-Which of the following reactions could be described by the above diagram?

Accepted Answer

A)  2 N2O2(g)   4 NO2(g) + O2(g) 
B)  H2(g) + CO2(g)   CO(g) + H2O(g) 
C)  PCl5(g)   PCl3(g) + Cl2(g) 
D)  2 NO(g) + Br2(g)   2 NOBr(g) 
E)  2 O3(g)   3 O2(g) 
A)  2 N2O2(g)   4 NO2(g) + O2(g) 
B)  H2(g) + CO2(g)   CO(g) + H2O(g) 
C)  PCl5(g)   PCl3(g) + Cl2(g) 
D)  2 NO(g) + Br2(g)   2 NOBr(g) 
E)  2 O3(g)   3 O2(g)

Question 2

Which of the following initial concentrations of reactants and products will cause the reaction to proceed to the right in order to establish equilibrium? 
2 NO2(g)   2 NO(g) + O2(g) Kc=3.4*10 -F 7 (at 200   C)

Accepted Answer

A)     
B)     
C)     
D)      
E)  none of these 
A)     
B)     
C)     
D)      
E)  none of these

Question 3

At equilibrium, ______________.

Accepted Answer

A)  all chemical processes have ceased. 
B)  the rate of the forward reaction equals that of the reverse. 
C)  the rate constant for the forward reaction equals that of the reverse. 
D)  $\underline{\text{  both }}$  the rate of the forward reaction equals that of the reverse $\underline{\text{  and }}$  the rate constant for the forward reaction equals that of the reverse. 
E)  none of the above 
A)  all chemical processes have ceased. 
B)  the rate of the forward reaction equals that of the reverse. 
C)  the rate constant for the forward reaction equals that of the reverse. 
D)  $\underline{\text{  both }}$  the rate of the forward reaction equals that of the reverse $\underline{\text{  and }}$  the rate constant for the forward reaction equals that of the reverse. 
E)  none of the above

Question 4

Calculate the COCl2, CO, and Cl2 concentrations when the following gas-phase reaction reaches equilibrium at 300°C.

Accepted Answer

[CO] = [Cl

Question 5

A solution is prepared in which the Pb2+ ion concentration is 0.020 M and the Br- ion concentration is 0.010 M. Which of the following statements is true given that Ksp for PbBr2 is 7.9 x 10-5?

Accepted Answer

A)  No PbBr2(s) will precipitate because Qspsp. 
B)  No PbBr2(s) will precipitate because Qsp>Ksp. 
C)  PbBr2 can only be formed from the reaction of Pb(s) with Br2(l). 
D)  A precipitate of PbBr2(s) will form because Qsp>Ksp. 
E)  Insufficient data is given to make a prediction about whether a precipitate will form or not. 
A)  No PbBr2(s) will precipitate because Qspsp. 
B)  No PbBr2(s) will precipitate because Qsp>Ksp. 
C)  PbBr2 can only be formed from the reaction of Pb(s) with Br2(l). 
D)  A precipitate of PbBr2(s) will form because Qsp>Ksp. 
E)  Insufficient data is given to make a prediction about whether a precipitate will form or not.

Question 6

What would happen to the extent of the decomposition of PCl5 at a given temperature if the pressure on the system were decreased by increasing the volume of the container at a constant temperature?

PCl5(g)   PCl3(g) + Cl2(g)

Accepted Answer

A)  It would increase. 
B)  It would decrease. 
C)  It would remain constant. 
D)  Not enough information is given to determine this. 
A)  It would increase. 
B)  It would decrease. 
C)  It would remain constant. 
D)  Not enough information is given to determine this.

Question 7

Assume that the equilibrium constants for the following reactions are known.

2 SO2(g) + O2(g)   2 SO3(g) &emsp; K1
2 CO(g) + O2(g)   2 CO2(g) &emsp; K2
What is the equilibrium constant for the following reaction?
2 SO2(g) + 2 CO2(g)   2 SO3(g) + 2 CO(g)

Accepted Answer

A)  K = K1 x K2 
B)  K = K1/K2 
C)  K = K2/K1 
D)  K = K1 + K2 
E)  K = K1 - K2 
A)  K = K1 x K2 
B)  K = K1/K2 
C)  K = K2/K1 
D)  K = K1 + K2 
E)  K = K1 - K2

Question 8

A 0.100 M sample of SO2 reacts with 0.060 M O2 to produce SO3 by the reaction shown below. There was no SO3 present initially. The concentration of O2 measured at equilibrium is found to be 0.020 M. What are the equilibrium concentrations of SO2 and SO3?

2 SO2(g) + O2(g)   2 SO3(g)

Accepted Answer

A)  [SO2] = 0.040M, [SO3] = 0.060M 
B)  [SO2] = 0.080M, [SO3] = 0.080M 
C)  [SO2] = 0.080M, [SO3] = 0.120M 
D)  [SO2] = 0.020M, [SO3] = 0.080M 
E)  none of these 
A)  [SO2] = 0.040M, [SO3] = 0.060M 
B)  [SO2] = 0.080M, [SO3] = 0.080M 
C)  [SO2] = 0.080M, [SO3] = 0.120M 
D)  [SO2] = 0.020M, [SO3] = 0.080M 
E)  none of these

Question 9

What is the concentration of Ag+ (mol/L) ion that results from saturating a 0.10 M NaBr solution with AgBr? 
The Ksp of AgBr is 5.0 x 10-13.

Accepted Answer

A)  5.0 x 10-12 M 
B)  2.2 x 10-6 M 
C)  0.10 M 
D)  1.2 x 10-11 M 
E)  none of the above 
A)  5.0 x 10-12 M 
B)  2.2 x 10-6 M 
C)  0.10 M 
D)  1.2 x 10-11 M 
E)  none of the above

Question 10

Which of the following equations describes the relationship between the solubility product for Ag2SO4 and the solubility of this compound?

Accepted Answer

A)  Ksp = 4 $\Delta$ C3 
B)  Ksp = 2 $\Delta$ C 
C)  Ksp = 4 $\Delta$ C2 
D)  Ksp =  $\Delta$ C3 
E)  none of the above 
A)  Ksp = 4 $\Delta$ C3 
B)  Ksp = 2 $\Delta$ C 
C)  Ksp = 4 $\Delta$ C2 
D)  Ksp =  $\Delta$ C3 
E)  none of the above

Question 11

Calculate the concentrations of all reactants and products when a mixture 
that is initially 0.10 M in N2, H2, and NH3 comes to equilibrium at 600 K.

N2(g) + 3 H2(g)   2 NH3(g) &emsp; Kc = 0.045

Accepted Answer

[NH₃] @#LAT-DLM& 1

Question 12

The following reactions are at equilibrium. Beside each reaction is a change that is made to the system which may cause a shift in equilibrium. Which of the reactions will shift its equilibrium toward the products?

Accepted Answer

A)  N2(g) + O2(g)   2 NO(g) &emsp; the concentration of NO is increased 
B)  PF5(g)   PF3(g) + F2(g) &emsp; the concentration of F2 is increased 
C)  Cl2(g) + 3 F2(g)   2 ClF3(g) &emsp; the concentration of Cl2 is decreased 
D)  2 SO3(g)   2 SO2(g) + O2(g) &emsp; the concentration of SO2 is decreased 
E)  none of these 
A)  N2(g) + O2(g)   2 NO(g) &emsp; the concentration of NO is increased 
B)  PF5(g)   PF3(g) + F2(g) &emsp; the concentration of F2 is increased 
C)  Cl2(g) + 3 F2(g)   2 ClF3(g) &emsp; the concentration of Cl2 is decreased 
D)  2 SO3(g)   2 SO2(g) + O2(g) &emsp; the concentration of SO2 is decreased 
E)  none of these

Question 13

What is the solubility in moles/L of CaF2 in water given that the Ksp is 4.0 x 10 - 11?

Accepted Answer

A)  2.2 x 10  - 4 
B)  4.0 x 10 - 11 
C)  3.5 x 10 - 4 
D)  6.0 x 10 - 5 
E)  2.0 x 10 - 11 
A)  2.2 x 10  - 4 
B)  4.0 x 10 - 11 
C)  3.5 x 10 - 4 
D)  6.0 x 10 - 5 
E)  2.0 x 10 - 11

Question 14

Assume an equilibrium constant Kc = 1.7 x 10-2 for the reaction:

N2(g) + 3 H2(g)   2 NH3(g)
Calculate (to a first approximation) the equilibrium concentrations of NH3, H2 and N2 when 0.10 moles per liter each of N2 and H2 are mixed and allowed to react to equilibrium.

Accepted Answer

NH₃ = 1.3

Question 15

If the Ksp of PbBr2 is 8.9 x 10-6, what is the solubility of PbBr2(s) in moles/L?

Accepted Answer

A)  8.9 x 10 - 6 
B)  1.3 x 10S1U1P1 -2S1S1P0 
C)  3.3 x 10 - 3 
D)  0.21 
E)  none of the above 
A)  8.9 x 10 - 6 
B)  1.3 x 10S1U1P1 -2S1S1P0 
C)  3.3 x 10 - 3 
D)  0.21 
E)  none of the above

Question 16

What is the correct solubility constant expression for AgCl(s)?

Accepted Answer

A)  Ksp = [Ag+][Cl - ] 
B)  Ksp = [Ag+] + [Cl - ]  
C)  Ksp =  [Ag+]/[Cl - ] 
D)  Ksp =  [Ag][Cl] 
E)  none of the above 
A)  Ksp = [Ag+][Cl - ] 
B)  Ksp = [Ag+] + [Cl - ]  
C)  Ksp =  [Ag+]/[Cl - ] 
D)  Ksp =  [Ag][Cl] 
E)  none of the above

Question 17

What is the correct solubility constant expression for PbSO4?

Accepted Answer

A)    
B)  Ksp =  [Pb2+][SO22-][O2]  
C)  Ksp =  [Pb2+][SO42-] 
D)    
E)  none of the above 
A)    
B)  Ksp =  [Pb2+][SO22-][O2]  
C)  Ksp =  [Pb2+][SO42-] 
D)    
E)  none of the above

Question 18

For the reaction shown below, at equilibrium
I2(g) + Br2(g)   2IBr(g) &emsp; Kc = 1.1 x 102

Accepted Answer

A)  Reactants and products will be present in approximately equal concentrations. 
B)  Reactants will be favored. 
C)  Products will be favored. 
D)  Insufficient information is given to decide. 
E)  It is impossible for the reaction to reach equilibrium. 
A)  Reactants and products will be present in approximately equal concentrations. 
B)  Reactants will be favored. 
C)  Products will be favored. 
D)  Insufficient information is given to decide. 
E)  It is impossible for the reaction to reach equilibrium.

Question 19

What is the effect of increasing the temperature on the following exothermic reaction?

2 CO(g) + O2(g)   2 CO2(g)

Accepted Answer

A)  The equilibrium will shift to the right. 
B)  The equilibrium will shift to the left. 
C)  The partial pressure of CO2 will increase. 
D)  The partial pressure of O2 will decrease. 
E)  It will have no effect. 
A)  The equilibrium will shift to the right. 
B)  The equilibrium will shift to the left. 
C)  The partial pressure of CO2 will increase. 
D)  The partial pressure of O2 will decrease. 
E)  It will have no effect.

Question 20

The following reactions are at equilibrium. Which of the reactions will shift its equilibrium toward the reactant side if the pressure is increased while holding the temperature constant?

Accepted Answer

A)  2 NO(g) + 2 H2(g)   N2(g) + 2 H2O(g) 
B)  2 NOCl(g)   2 NO(g) + Cl2(g) 
C)  2 NO(g) + O2(g)   2 NO2(g) 
D)  N2(g) + O2(g)   2 NO(g) 
E)  NO(g) + NO2(g)   N2O3(g) 
A)  2 NO(g) + 2 H2(g)   N2(g) + 2 H2O(g) 
B)  2 NOCl(g)   2 NO(g) + Cl2(g) 
C)  2 NO(g) + O2(g)   2 NO2(g) 
D)  N2(g) + O2(g)   2 NO(g) 
E)  NO(g) + NO2(g)   N2O3(g)

-Which of the following reactions could be described by the above diagram?

Which of the following initial concentrations of reactants and products will cause the reaction to proceed to the right in order to establish equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g) K_c=3.4*10 ^-F ⁷ (at 200 C)

At equilibrium, ______________.

Calculate the COCl₂, CO, and Cl₂ concentrations when the following gas-phase reaction reaches equilibrium at 300°C.

A solution is prepared in which the Pb²⁺ ion concentration is 0.020 M and the Br^- ion concentration is 0.010 M. Which of the following statements is true given that K_sp for PbBr₂ is 7.9 x 10^-5?

What would happen to the extent of the decomposition of PCl₅ at a given temperature if the pressure on the system were decreased by increasing the volume of the container at a constant temperature? PCl₅(g) PCl₃(g) + Cl₂(g)

Assume that the equilibrium constants for the following reactions are known. 2 SO₂(g) + O₂(g) 2 SO₃(g) K₁ 2 CO(g) + O₂(g) 2 CO₂(g) K₂ What is the equilibrium constant for the following reaction? 2 SO₂(g) + 2 CO₂(g) 2 SO₃(g) + 2 CO(g)

A 0.100 M sample of SO₂ reacts with 0.060 M O₂ to produce SO₃ by the reaction shown below. There was no SO₃ present initially. The concentration of O₂ measured at equilibrium is found to be 0.020 M. What are the equilibrium concentrations of SO₂ and SO₃? 2 SO₂(g) + O₂(g) 2 SO₃(g)

What is the concentration of Ag⁺ (mol/L) ion that results from saturating a 0.10 M NaBr solution with AgBr? The K_sp of AgBr is 5.0 x 10^-13.

Which of the following equations describes the relationship between the solubility product for Ag₂SO₄ and the solubility of this compound?

Calculate the concentrations of all reactants and products when a mixture that is initially 0.10 M in N₂, H₂, and NH₃ comes to equilibrium at 600 K. N₂(g) + 3 H₂(g) 2 NH₃(g) K_c = 0.045

The following reactions are at equilibrium. Beside each reaction is a change that is made to the system which may cause a shift in equilibrium. Which of the reactions will shift its equilibrium toward the products?

What is the solubility in moles/L of CaF₂ in water given that the K_sp is 4.0 x 10 ^- ¹¹?

Assume an equilibrium constant K_c = 1.7 x 10^-2 for the reaction: N₂(g) + 3 H₂(g) 2 NH₃(g) Calculate (to a first approximation) the equilibrium concentrations of NH₃, H₂ and N₂ when 0.10 moles per liter each of N₂ and H₂ are mixed and allowed to react to equilibrium.

If the K_sp of PbBr₂ is 8.9 x 10^-6, what is the solubility of PbBr₂(s) in moles/L?

What is the correct solubility constant expression for AgCl(s)?

What is the correct solubility constant expression for PbSO₄?

For the reaction shown below, at equilibrium I₂(g) + Br₂(g) 2IBr(g) K_c = 1.1 x 10²

What is the effect of increasing the temperature on the following exothermic reaction? 2 CO(g) + O₂(g) 2 CO₂(g)

The following reactions are at equilibrium. Which of the reactions will shift its equilibrium toward the reactant side if the pressure is increased while holding the temperature constant?

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Exam 10: An Introduction to Kinetics and Equilibrium

-Which of the following reactions could be described by the above diagram?

Which of the following initial concentrations of reactants and products will cause the reaction to proceed to the right in order to establish equilibrium? 2 NO2(g) 2 NO(g) + O2(g) Kc=3.4*10 -F 7 (at 200 C)

At equilibrium, ______________.

Calculate the COCl2, CO, and Cl2 concentrations when the following gas-phase reaction reaches equilibrium at 300°C.

A solution is prepared in which the Pb2+ ion concentration is 0.020 M and the Br- ion concentration is 0.010 M. Which of the following statements is true given that Ksp for PbBr2 is 7.9 x 10-5?

What would happen to the extent of the decomposition of PCl5 at a given temperature if the pressure on the system were decreased by increasing the volume of the container at a constant temperature? PCl5(g) PCl3(g) + Cl2(g)

Assume that the equilibrium constants for the following reactions are known. 2 SO2(g) + O2(g) 2 SO3(g) K1 2 CO(g) + O2(g) 2 CO2(g) K2 What is the equilibrium constant for the following reaction? 2 SO2(g) + 2 CO2(g) 2 SO3(g) + 2 CO(g)

A 0.100 M sample of SO2 reacts with 0.060 M O2 to produce SO3 by the reaction shown below. There was no SO3 present initially. The concentration of O2 measured at equilibrium is found to be 0.020 M. What are the equilibrium concentrations of SO2 and SO3? 2 SO2(g) + O2(g) 2 SO3(g)

What is the concentration of Ag+ (mol/L) ion that results from saturating a 0.10 M NaBr solution with AgBr? The Ksp of AgBr is 5.0 x 10-13.

Which of the following equations describes the relationship between the solubility product for Ag2SO4 and the solubility of this compound?

Calculate the concentrations of all reactants and products when a mixture that is initially 0.10 M in N2, H2, and NH3 comes to equilibrium at 600 K. N2(g) + 3 H2(g) 2 NH3(g) Kc = 0.045

The following reactions are at equilibrium. Beside each reaction is a change that is made to the system which may cause a shift in equilibrium. Which of the reactions will shift its equilibrium toward the products?

What is the solubility in moles/L of CaF2 in water given that the Ksp is 4.0 x 10 - 11?

Assume an equilibrium constant Kc = 1.7 x 10-2 for the reaction: N2(g) + 3 H2(g) 2 NH3(g) Calculate (to a first approximation) the equilibrium concentrations of NH3, H2 and N2 when 0.10 moles per liter each of N2 and H2 are mixed and allowed to react to equilibrium.

If the Ksp of PbBr2 is 8.9 x 10-6, what is the solubility of PbBr2(s) in moles/L?

What is the correct solubility constant expression for AgCl(s)?

What is the correct solubility constant expression for PbSO4?

For the reaction shown below, at equilibrium I2(g) + Br2(g) 2IBr(g) Kc = 1.1 x 102

What is the effect of increasing the temperature on the following exothermic reaction? 2 CO(g) + O2(g) 2 CO2(g)

The following reactions are at equilibrium. Which of the reactions will shift its equilibrium toward the reactant side if the pressure is increased while holding the temperature constant?

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Which of the following initial concentrations of reactants and products will cause the reaction to proceed to the right in order to establish equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g) K_c=3.4*10 ^-F ⁷ (at 200 C)

Calculate the COCl₂, CO, and Cl₂ concentrations when the following gas-phase reaction reaches equilibrium at 300°C.

A solution is prepared in which the Pb²⁺ ion concentration is 0.020 M and the Br^- ion concentration is 0.010 M. Which of the following statements is true given that K_sp for PbBr₂ is 7.9 x 10^-5?

What would happen to the extent of the decomposition of PCl₅ at a given temperature if the pressure on the system were decreased by increasing the volume of the container at a constant temperature? PCl₅(g) PCl₃(g) + Cl₂(g)

Assume that the equilibrium constants for the following reactions are known. 2 SO₂(g) + O₂(g) 2 SO₃(g) K₁ 2 CO(g) + O₂(g) 2 CO₂(g) K₂ What is the equilibrium constant for the following reaction? 2 SO₂(g) + 2 CO₂(g) 2 SO₃(g) + 2 CO(g)

What is the concentration of Ag⁺ (mol/L) ion that results from saturating a 0.10 M NaBr solution with AgBr? The K_sp of AgBr is 5.0 x 10^-13.

Which of the following equations describes the relationship between the solubility product for Ag₂SO₄ and the solubility of this compound?

Calculate the concentrations of all reactants and products when a mixture that is initially 0.10 M in N₂, H₂, and NH₃ comes to equilibrium at 600 K. N₂(g) + 3 H₂(g) 2 NH₃(g) K_c = 0.045

What is the solubility in moles/L of CaF₂ in water given that the K_sp is 4.0 x 10 ^- ¹¹?

Assume an equilibrium constant K_c = 1.7 x 10^-2 for the reaction: N₂(g) + 3 H₂(g) 2 NH₃(g) Calculate (to a first approximation) the equilibrium concentrations of NH₃, H₂ and N₂ when 0.10 moles per liter each of N₂ and H₂ are mixed and allowed to react to equilibrium.

If the K_sp of PbBr₂ is 8.9 x 10^-6, what is the solubility of PbBr₂(s) in moles/L?

What is the correct solubility constant expression for PbSO₄?

For the reaction shown below, at equilibrium I₂(g) + Br₂(g) 2IBr(g) K_c = 1.1 x 10²

What is the effect of increasing the temperature on the following exothermic reaction? 2 CO(g) + O₂(g) 2 CO₂(g)