Question 1

What is the Ksp of SrF2(s) if 0.073 g of SrF2 dissolves in 1.00 liter of solution?

Accepted Answer

A)  5.8 x 10 - 4 
B)  1.7 x 10 - 3 
C)  1.6 x 10 - 3 
D)  7.8 x 10 - 10 
E)  none of the above 
A)  5.8 x 10 - 4 
B)  1.7 x 10 - 3 
C)  1.6 x 10 - 3 
D)  7.8 x 10 - 10 
E)  none of the above

Question 2

The following reaction is at equilibrium. Which of the conditions listed below will cause the reaction to shift toward the products?
2 SO3(g) + 2 Cl2(g)   2 SO2Cl2(g)+ O2(g)

Accepted Answer

A)  The concentration of O2 is increased. 
B)  The concentration of SO2Cl2 is decreased. 
C)  The concentration of SO3 is decreased. 
D)  The pressure is decreased. 
E)  none of these 
A)  The concentration of O2 is increased. 
B)  The concentration of SO2Cl2 is decreased. 
C)  The concentration of SO3 is decreased. 
D)  The pressure is decreased. 
E)  none of these

Question 3

The following reaction was carried out at 250C with the initial concentration of NO2 being 0.70 M and no NO(g) or O2(g) initially present. At equilibrium the NO2 concentration was found to be 0.28 M. Calculate Kc for the reaction.
2NO2(g)   2NO(g) + O2(g)

Accepted Answer

A)  0.47 
B)  0.94 
C)  1.9 
D)  0.14 
E)  2.1 
A)  0.47 
B)  0.94 
C)  1.9 
D)  0.14 
E)  2.1

Question 4

-What happens to the rate of the reaction as time passes in the equilibrium region of the graph above?

Accepted Answer

A)  the rate increases 
B)  the rate decreases 
C)  the rate remains constant 
D)  cannot be determined from the graph 
A)  the rate increases 
B)  the rate decreases 
C)  the rate remains constant 
D)  cannot be determined from the graph

Question 5

Use the following graph for answering 
  
-Using the above graph determine the balanced chemical equation.

Accepted Answer

A)  3 A + B   2 C 
B)  5 A + 3 B   2 C 
C)  2 C + 3 B   5 A 
D)  A + B   C 
E)  none of these 
A)  3 A + B   2 C 
B)  5 A + 3 B   2 C 
C)  2 C + 3 B   5 A 
D)  A + B   C 
E)  none of these

Question 6

If 1.3 x 10 - 5 moles of AgCl will dissolve in 1.0 liter of water at 25-C, what is the Ksp of AgCl?

Accepted Answer

A)  5.1 x 10  - 9 
B)  3.6 x 10 - 3 
C)  6.4 x 10 - 5 
D)  1.3 x 10 - 5 
E)  1.7 x 10-10 
A)  5.1 x 10  - 9 
B)  3.6 x 10 - 3 
C)  6.4 x 10 - 5 
D)  1.3 x 10 - 5 
E)  1.7 x 10-10

Question 7

For the reaction below, 0.0500 moles of ethyl acetate are allowed to react with 0.200 moles of water. At equilibrium it is found that 0.0300 moles of acetic acid have been produced. How many moles of ethyl acetate remain at equilibrium?

Accepted Answer

A)  0.0100 moles 
B)  0.0300 moles 
C)  0.0500 moles 
D)  0.170 moles 
E)  none of these 
A)  0.0100 moles 
B)  0.0300 moles 
C)  0.0500 moles 
D)  0.170 moles 
E)  none of these

Question 8

The following chemical reaction has reached equilibrium. Which of the changes listed below would cause the equilibrium to shift back toward the reactants? 
N2(g) + 3 H2(g)   2 NH3(g) &emsp;  $\Delta$ H = -92.2 kJ/molrxn

Accepted Answer

A)  increasing the pressure 
B)  increasing the concentration of N2 
C)  increasing the temperature 
D)  decreasing the concentration of NH3 
E)  none of these 
A)  increasing the pressure 
B)  increasing the concentration of N2 
C)  increasing the temperature 
D)  decreasing the concentration of NH3 
E)  none of these

Question 9

For the reaction:
CO(g) + Cl2(g)   COCl2(g)
Kf is 1x 107 M-1-s-1 and kr = 2 x 102 s-1.
 What is the equilibrium constant for the reaction?

Accepted Answer

A)  2 x 10-5 
B)  5 
C)  5 x 104 
D)  2 x 109 
E)  none of these 
A)  2 x 10-5 
B)  5 
C)  5 x 104 
D)  2 x 109 
E)  none of these

Question 10

Use the following graph for answering 
  
-Which of the following will be true of the equilibrium constant, Kc, for the reaction described in the above graph?

Accepted Answer

A)  Kc  $\approx$  1 
B)  Kc  $\approx$  0 
C)  Kc c > 1 
E)  cannot be determined from graph 
A)  Kc  $\approx$  1 
B)  Kc  $\approx$  0 
C)  Kc c > 1 
E)  cannot be determined from graph

Question 11

Calculate the NO, NO2, and O2 concentrations in the following gas-phase reaction at equilibrium at 200°C.

Accepted Answer

[NO₂] = 0.1

Question 12

What would happen if F2 was removed from the following reaction while it was at equilibrium?

Cl2(g) + 3 F2(g)   2 ClF3(g)

Accepted Answer

A)  The concentration of Cl2 would increase as the reaction returned to equilibrium. 
B)  The concentration of both Cl2 and F2 would increase as the reaction returned to equilibrium. 
C)  The concentration of Cl2 would decrease as the reaction returned to equilibrium. 
D)  The concentration of both Cl2 and F2 would decrease as the reaction returned to equilibrium. 
E)  The concentration of both F2 and Cl2 would remain the same because the reaction would be at equilibrium. 
A)  The concentration of Cl2 would increase as the reaction returned to equilibrium. 
B)  The concentration of both Cl2 and F2 would increase as the reaction returned to equilibrium. 
C)  The concentration of Cl2 would decrease as the reaction returned to equilibrium. 
D)  The concentration of both Cl2 and F2 would decrease as the reaction returned to equilibrium. 
E)  The concentration of both F2 and Cl2 would remain the same because the reaction would be at equilibrium.

Question 13

Calculate the equilibrium concentrations of SO3, SO2, and O2 if 0.100 moles of SO3 in a 10-L flask decompose to form SO2 and O2 at 500 K.

2 SO3(g)   2 SO2(g) + O2(g) &emsp; Kc = 1.4 x 10-11

Accepted Answer

[O₂] = 7.0

Question 14

For the following reaction
2 C2H6(g) + 7 O2(g)   4 CO2(g) + 6 H2O(g)

If the reaction mixture initially contained all species at the same initial concentration, C, and if the concentration of O2 at equilibrium was expressed as [O2] = C + 7  $\Delta$ C , then the concentration of H2O at equilibrium would be correctly expressed as [H2O] =

Accepted Answer

A)  C +  $\Delta$ C 
B)  C -  $\Delta$ C 
C)  C + 6 $\Delta$ C 
D)  C - 6 $\Delta$ C 
E)  none of the above 
A)  C +  $\Delta$ C 
B)  C -  $\Delta$ C 
C)  C + 6 $\Delta$ C 
D)  C - 6 $\Delta$ C 
E)  none of the above

What is the K_sp of SrF₂(s) if 0.073 g of SrF₂ dissolves in 1.00 liter of solution?

The following reaction is at equilibrium. Which of the conditions listed below will cause the reaction to shift toward the products? 2 SO₃(g) + 2 Cl₂(g) 2 SO₂Cl₂(g)+ O₂(g)

The following reaction was carried out at 25⁰C with the initial concentration of NO₂ being 0.70 M and no NO(g) or O₂(g) initially present. At equilibrium the NO₂concentration was found to be 0.28 M. Calculate K_c for the reaction. 2NO₂(g) 2NO(g) + O₂(g)

-What happens to the rate of the reaction as time passes in the equilibrium region of the graph above?

Use the following graph for answering -Using the above graph determine the balanced chemical equation.

If 1.3 x 10 ^- ⁵ moles of AgCl will dissolve in 1.0 liter of water at 25-C, what is the K_sp of AgCl?

For the reaction below, 0.0500 moles of ethyl acetate are allowed to react with 0.200 moles of water. At equilibrium it is found that 0.0300 moles of acetic acid have been produced. How many moles of ethyl acetate remain at equilibrium?

For the reaction: CO(g) + Cl₂(g) COCl₂(g) K_f is 1x 10⁷ M^-1-s^-1 and k_r = 2 x 10² s^-1. What is the equilibrium constant for the reaction?

Use the following graph for answering -Which of the following will be true of the equilibrium constant, K_c, for the reaction described in the above graph?

Calculate the NO, NO₂, and O₂ concentrations in the following gas-phase reaction at equilibrium at 200°C.

What would happen if F₂ was removed from the following reaction while it was at equilibrium? Cl₂(g) + 3 F₂(g) 2 ClF₃(g)

Calculate the equilibrium concentrations of SO₃, SO₂, and O₂ if 0.100 moles of SO₃ in a 10-L flask decompose to form SO₂ and O₂ at 500 K. 2 SO₃(g) 2 SO₂(g) + O₂(g) K_c = 1.4 x 10^-11

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

What is the Ksp of SrF2(s) if 0.073 g of SrF2 dissolves in 1.00 liter of solution?

The following reaction is at equilibrium. Which of the conditions listed below will cause the reaction to shift toward the products? 2 SO3(g) + 2 Cl2(g) 2 SO2Cl2(g)+ O2(g)

The following reaction was carried out at 250C with the initial concentration of NO2 being 0.70 M and no NO(g) or O2(g) initially present. At equilibrium the NO2 concentration was found to be 0.28 M. Calculate Kc for the reaction. 2NO2(g) 2NO(g) + O2(g)

-What happens to the rate of the reaction as time passes in the equilibrium region of the graph above?

Use the following graph for answering -Using the above graph determine the balanced chemical equation.

If 1.3 x 10 - 5 moles of AgCl will dissolve in 1.0 liter of water at 25-C, what is the Ksp of AgCl?

For the reaction below, 0.0500 moles of ethyl acetate are allowed to react with 0.200 moles of water. At equilibrium it is found that 0.0300 moles of acetic acid have been produced. How many moles of ethyl acetate remain at equilibrium?

The following chemical reaction has reached equilibrium. Which of the changes listed below would cause the equilibrium to shift back toward the reactants? N2(g) + 3 H2(g) 2 NH3(g) Δ\DeltaΔ H = -92.2 kJ/molrxn

For the reaction: CO(g) + Cl2(g) COCl2(g) Kf is 1x 107 M-1-s-1 and kr = 2 x 102 s-1. What is the equilibrium constant for the reaction?

Use the following graph for answering -Which of the following will be true of the equilibrium constant, Kc, for the reaction described in the above graph?

Calculate the NO, NO2, and O2 concentrations in the following gas-phase reaction at equilibrium at 200°C.

What would happen if F2 was removed from the following reaction while it was at equilibrium? Cl2(g) + 3 F2(g) 2 ClF3(g)

Calculate the equilibrium concentrations of SO3, SO2, and O2 if 0.100 moles of SO3 in a 10-L flask decompose to form SO2 and O2 at 500 K. 2 SO3(g) 2 SO2(g) + O2(g) Kc = 1.4 x 10-11

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

What is the K_sp of SrF₂(s) if 0.073 g of SrF₂ dissolves in 1.00 liter of solution?

The following reaction is at equilibrium. Which of the conditions listed below will cause the reaction to shift toward the products? 2 SO₃(g) + 2 Cl₂(g) 2 SO₂Cl₂(g)+ O₂(g)

The following reaction was carried out at 25⁰C with the initial concentration of NO₂ being 0.70 M and no NO(g) or O₂(g) initially present. At equilibrium the NO₂concentration was found to be 0.28 M. Calculate K_c for the reaction. 2NO₂(g) 2NO(g) + O₂(g)

If 1.3 x 10 ^- ⁵ moles of AgCl will dissolve in 1.0 liter of water at 25-C, what is the K_sp of AgCl?

For the reaction: CO(g) + Cl₂(g) COCl₂(g) K_f is 1x 10⁷ M^-1-s^-1 and k_r = 2 x 10² s^-1. What is the equilibrium constant for the reaction?

Use the following graph for answering -Which of the following will be true of the equilibrium constant, K_c, for the reaction described in the above graph?

Calculate the NO, NO₂, and O₂ concentrations in the following gas-phase reaction at equilibrium at 200°C.

What would happen if F₂ was removed from the following reaction while it was at equilibrium? Cl₂(g) + 3 F₂(g) 2 ClF₃(g)

Calculate the equilibrium concentrations of SO₃, SO₂, and O₂ if 0.100 moles of SO₃ in a 10-L flask decompose to form SO₂ and O₂ at 500 K. 2 SO₃(g) 2 SO₂(g) + O₂(g) K_c = 1.4 x 10^-11