Question 1

Pure and pure are excluded from equilibrium- constant expressions.

Accepted Answer

The answer of Pure and pure are excluded from equilibrium-...

Question 2

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction:
PCl3 (g) + Cl2 (g) -PCl5 (g)
An equilibrium mixture at 450 K contains PPCl3 = 0.202 atm,
PCl2 = 0.256 atm, and
PPCl5 = 3.45 atm. What is the value of Kp at this temperature?

Accepted Answer

A)  1.50 × 10- 2 
B)  66.8 
C)  2.99 
D)  7.54 
E)  1.78 × 10- 1 
A)  1.50 × 10- 2 
B)  66.8 
C)  2.99 
D)  7.54 
E)  1.78 × 10- 1

Question 3

Consider the following equilibrium.
 
The equilibrium cannot be established when _ _ is/are placed in a 1.0- L container.

Accepted Answer

A) 0.50 mol O2 (g) and 0.50 mol SO3 (g) 
B) 0.75 mol SO2 (g) 
C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g) 
D) 1.0 mol SO3 (g) 
E) 0.25 mol SO2 (g) and 0.25 mol O2 (g) 
A) 0.50 mol O2 (g) and 0.50 mol SO3 (g) 
B) 0.75 mol SO2 (g) 
C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g) 
D) 1.0 mol SO3 (g) 
E) 0.25 mol SO2 (g) and 0.25 mol O2 (g)

Question 4

What role did Karl Bosch play in development of the Haber- Bosch process?

Accepted Answer

A) He originally isolated ammonia from camel dung and found a method for purifying it. 
B) He was the German industrialist who financed the research done by Haber. 
C) He discovered the reaction conditions necessary for formation of ammonia. 
D) He developed the equipment necessary for industrial production of ammonia. 
E) Haber was working in his lab with his instructor at the time he worked out the process. 
A) He originally isolated ammonia from camel dung and found a method for purifying it. 
B) He was the German industrialist who financed the research done by Haber. 
C) He discovered the reaction conditions necessary for formation of ammonia. 
D) He developed the equipment necessary for industrial production of ammonia. 
E) Haber was working in his lab with his instructor at the time he worked out the process.

Question 5

Consider the following chemical reaction:
H2 (g) + I2 (g)   2HI (g)
At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M,
0)033 M, and 0.55 M, respectively. The value of Keq for this reaction is .

Accepted Answer

A)  9.0 × 10- 3  
B)  61 
C)  23 
D)  111 
E)  6.1 
A)  9.0 × 10- 3  
B)  61 
C)  23 
D)  111 
E)  6.1

Question 6

The equilibrium- constant expression for the reaction 
 
is given by

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 7

The equilibrium- constant expression for a reaction written in one direction is the
of the one for the reaction written for the reverse direction.

Accepted Answer

The answer of The equilibrium- constant expression for a reaction...

Question 8

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is . (1) SO2 (g) + (1/2) O2 (g)   SO3 (g)
(2) 2SO3 (g)   2SO2 (g) + O2 (g)

Accepted Answer

A)  1/K2  
B)  K2  
C)  2K 
D)  - K2  
E)  1/2K 
A)  1/K2  
B)  K2  
C)  2K 
D)  - K2  
E)  1/2K

Question 9

The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is KS1U1B1eqS1U1B0= .

Accepted Answer

A) kS1U1B1fS1U1B0S1U1B1 S1U1B0+ kS1U1B1rS1U1B0 
B)  kS1U1B1fS1U1B0kS1U1B1rS1U1B0 
C)  kS1U1B1fS1U1B0/kS1U1B1rS1U1B0 
D)  kS1U1B1rS1U1B0/kS1U1B1fS1U1B0 
E)  kS1U1B1f S1U1B0- kS1U1B1rS1U1B0 
A) kS1U1B1fS1U1B0S1U1B1 S1U1B0+ kS1U1B1rS1U1B0 
B)  kS1U1B1fS1U1B0kS1U1B1rS1U1B0 
C)  kS1U1B1fS1U1B0/kS1U1B1rS1U1B0 
D)  kS1U1B1rS1U1B0/kS1U1B1fS1U1B0 
E)  kS1U1B1f S1U1B0- kS1U1B1rS1U1B0

Question 10

The value of Keq for the following reaction is 0.25:

Accepted Answer

A)  0.12 
B)  0.062 
C)  16 
D)  0.25 
E)  0.50 
A)  0.12 
B)  0.062 
C)  16 
D)  0.25 
E)  0.50

Question 11

Nitrosyl bromide decomposes according to the following equation.  
A sample of NOBr (0.64 mol) was placed in a 1.00- L flask containing no NO or Br2. At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?

Accepted Answer

A)  0.46, 0.23 
B)  0.46, 0.46 
C)  0.18, 0.360 
D)  0.18, 0.18 
E)  0.18, 0.090 
A)  0.46, 0.23 
B)  0.46, 0.46 
C)  0.18, 0.360 
D)  0.18, 0.18 
E)  0.18, 0.090

Question 12

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C.

Accepted Answer

A)  5.66 × 10- 3
  
B)  0.150 
C)  0.0752 
D)  - 0.0752 
E)  13.3 
A)  5.66 × 10- 3
  
B)  0.150 
C)  0.0752 
D)  - 0.0752 
E)  13.3

Question 13

How is the reaction quotient used to determine whether a system is at equilibrium?

Accepted Answer

A) The reaction is at equilibrium when Q > Keq. 
B) The reaction is at equilibrium when Q = Keq. 
C) The reaction quotient must be satisfied for equilibrium to be achieved. 
D) The reaction is at equilibrium when Q eq. 
E) At equilibrium, the reaction quotient is undefined. 
A) The reaction is at equilibrium when Q > Keq. 
B) The reaction is at equilibrium when Q = Keq. 
C) The reaction quotient must be satisfied for equilibrium to be achieved. 
D) The reaction is at equilibrium when Q eq. 
E) At equilibrium, the reaction quotient is undefined.

Question 14

Which one of the following is true concerning the Haber process?

Accepted Answer

A) It is a process used for the synthesis of ammonia. 
B) It is an industrial synthesis of sodium chloride that was discovered by Karl Haber. 
C) It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances. 
D) It is another way of stating LeChatelier's principle. 
E) It is a process for the synthesis of elemental chlorine. 
A) It is a process used for the synthesis of ammonia. 
B) It is an industrial synthesis of sodium chloride that was discovered by Karl Haber. 
C) It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances. 
D) It is another way of stating LeChatelier's principle. 
E) It is a process for the synthesis of elemental chlorine.

Question 15

At 22 °C, Kp = 0.070 for the equilibrium:
NH4HS (s)   NH3 (g) + H2S (g)
A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.

Accepted Answer

A)  0.070 
B)  0.26 
C)  3.8 
D)  0.52 
E)  4.9 × 10- 3 
A)  0.070 
B)  0.26 
C)  3.8 
D)  0.52 
E)  4.9 × 10- 3

Question 16

At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) -2SO3 (g)
At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is _ atm.

Accepted Answer

A)  6.20 × 10- 4 
B)  192 
C)  40.2 
D)  82.0 
E)  4.21 × 10- 3 
A)  6.20 × 10- 4 
B)  192 
C)  40.2 
D)  82.0 
E)  4.21 × 10- 3

Question 17

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C.
2Cl2 (g) + 2H2O (g)   4HCl (g) + O2 (g)
What is the value of Keq at this temperature for the following reaction?
Cl2 (g) + H2O (g)   2HCl (g) + 1 O2 (g)

Accepted Answer

A)  0.274 
B)  5.66 × 10- 3 
C)  0.150 
D)  0.0752 
E)  0.0376 
A)  0.274 
B)  5.66 × 10- 3 
C)  0.150 
D)  0.0752 
E)  0.0376

Question 18

Which one of the following will change the value of an equilibrium constant?

Accepted Answer

A) adding other substances that do not react with any of the species involved in the equilibrium 
B) varying the initial concentrations of products 
C) changing temperature 
D) varying the initial concentrations of reactants 
E) changing the volume of the reaction vessel 
A) adding other substances that do not react with any of the species involved in the equilibrium 
B) varying the initial concentrations of products 
C) changing temperature 
D) varying the initial concentrations of reactants 
E) changing the volume of the reaction vessel

Pure and pure are excluded from equilibrium- constant expressions.

Consider the following equilibrium. The equilibrium cannot be established when _ _ is/are placed in a 1.0- L container.

What role did Karl Bosch play in development of the Haber- Bosch process?

Consider the following chemical reaction: H₂(g) + I₂(g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.15 M, 0)033 M, and 0.55 M, respectively. The value of K_eqfor this reaction is .

The equilibrium- constant expression for the reaction is given by

The equilibrium- constant expression for a reaction written in one direction is the of the one for the reaction written for the reverse direction.

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is . (1) SO₂(g) + (1/2) O₂(g) SO₃(g) (2) 2SO₃(g) 2SO₂(g) + O₂(g)

The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is K_eq= .

The value of K_eqfor the following reaction is 0.25:

Nitrosyl bromide decomposes according to the following equation. A sample of NOBr (0.64 mol) was placed in a 1.00- L flask containing no NO or Br₂. At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br₂, respectively, are in the flask at equilibrium?

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C.

How is the reaction quotient used to determine whether a system is at equilibrium?

Which one of the following is true concerning the Haber process?

At 22 °C, K_p= 0.070 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains.

At 900 K, the equilibrium constant (K_p) for the following reaction is 0.345. 2SO₂+ O₂(g) -2SO₃(g) At equilibrium, the partial pressure of SO₂is 35.0 atm and that of O₂is 15.9 atm. The partial pressure of SO₃is _ atm.

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C. 2Cl₂(g) + 2H2O (g) 4HCl (g) + O₂(g) What is the value of K_eqat this temperature for the following reaction? Cl₂(g) + H₂O (g) 2HCl (g) +¹O₂(g)

Which one of the following will change the value of an equilibrium constant?

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Exam 15: Chemical Equilibrium

Pure and pure are excluded from equilibrium- constant expressions.

Consider the following equilibrium. The equilibrium cannot be established when _ _ is/are placed in a 1.0- L container.

What role did Karl Bosch play in development of the Haber- Bosch process?

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0)033 M, and 0.55 M, respectively. The value of Keq for this reaction is .

The equilibrium- constant expression for the reaction is given by

The equilibrium- constant expression for a reaction written in one direction is the of the one for the reaction written for the reverse direction.

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is . (1) SO2 (g) + (1/2) O2 (g) SO3 (g) (2) 2SO3 (g) 2SO2 (g) + O2 (g)

The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq= .

The value of Keq for the following reaction is 0.25:

Nitrosyl bromide decomposes according to the following equation. A sample of NOBr (0.64 mol) was placed in a 1.00- L flask containing no NO or Br2. At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C.

How is the reaction quotient used to determine whether a system is at equilibrium?

Which one of the following is true concerning the Haber process?

At 22 °C, Kp = 0.070 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.

At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) -2SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is _ atm.

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? Cl2 (g) + H2O (g) 2HCl (g) + 1 O2 (g)

Which one of the following will change the value of an equilibrium constant?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

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Consider the following chemical reaction: H₂(g) + I₂(g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.15 M, 0)033 M, and 0.55 M, respectively. The value of K_eqfor this reaction is .

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is . (1) SO₂(g) + (1/2) O₂(g) SO₃(g) (2) 2SO₃(g) 2SO₂(g) + O₂(g)

The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is K_eq= .

The value of K_eqfor the following reaction is 0.25:

Nitrosyl bromide decomposes according to the following equation. A sample of NOBr (0.64 mol) was placed in a 1.00- L flask containing no NO or Br₂. At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br₂, respectively, are in the flask at equilibrium?

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C.

At 22 °C, K_p= 0.070 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains.

At 900 K, the equilibrium constant (K_p) for the following reaction is 0.345. 2SO₂+ O₂(g) -2SO₃(g) At equilibrium, the partial pressure of SO₂is 35.0 atm and that of O₂is 15.9 atm. The partial pressure of SO₃is _ atm.

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C. 2Cl₂(g) + 2H2O (g) 4HCl (g) + O₂(g) What is the value of K_eqat this temperature for the following reaction? Cl₂(g) + H₂O (g) 2HCl (g) +¹O₂(g)