Question 1

The equilibrium constant for the gas phase reaction 2SO2 (g)+ O2 (g)   2SO3 (g)
Is Keq = 2.80 × 102 at 999 K.At equilibrium,________.

Accepted Answer

A) products predominate 
B) reactants predominate 
C) roughly equal amounts of products and reactants are present 
D) only products are present 
E) only reactants are present 
A) products predominate 
B) reactants predominate 
C) roughly equal amounts of products and reactants are present 
D) only products are present 
E) only reactants are present

Question 2

Define the reaction quotient.

Accepted Answer

The number obtained by substit

Question 3

Le Châtelier's principle states that if a system at equilibrium is disturbed,then more reactants are produced.

Accepted Answer

A) True 
 B)False

Question 4

Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with   of N2O4.At equilibrium at 373 K,0.0055 mol of N2O4 remains.Keq for this reaction is ________.

Accepted Answer

A) 2.2 × 10-4 
B) 13 
C) 0.22 
D) 0.87 
E) 0.022 
A) 2.2 × 10-4 
B) 13 
C) 0.22 
D) 0.87 
E) 0.022

Question 5

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

Accepted Answer

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

Question 6

The value of Keq for the equilibrium H2 (g)+ I2 (g)   2HI (g)
Is 794 at 25 °C.At this temperature,what is the value of Keq for the equilibrium below?
HI (g)   1/2 H2 (g)+ 1/2 I2 (g)

Accepted Answer

A) 1588 
B) 28 
C) 397 
D) 0.035 
E) 0.0013 
A) 1588 
B) 28 
C) 397 
D) 0.035 
E) 0.0013

Question 7

The equilibrium constant for the gas phase reaction 2NH3 (g)   N2 (g)+ 3H2 (g)
Is Keq = 230 at 300 °C.At equilibrium,________.

Accepted Answer

A) products predominate 
B) reactants predominate 
C) roughly equal amounts of products and reactants are present 
D) only products are present 
E) only reactants are present 
A) products predominate 
B) reactants predominate 
C) roughly equal amounts of products and reactants are present 
D) only products are present 
E) only reactants are present

Question 8

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)   2NO (g)+   (g)
A sample of NOBr (0.64 mol)was placed in a 1.00-L flask containing no NO or   .At equilibrium the flask contained   of NOBr.How many moles of NO and   ,respectively,are in the flask at equilibrium?

Accepted Answer

A) 0.48, 0.24 
B) 0.48, 0.48 
C) 0.16, 0.08 
D) 0.16, 0.16 
E) 0.24, 0.42 
A) 0.48, 0.24 
B) 0.48, 0.48 
C) 0.16, 0.08 
D) 0.16, 0.16 
E) 0.24, 0.42

Question 9

Consider the following reaction at equilibrium. 2CO2 (g)   2CO (g)+ O2 (g)ΔH° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g)can be maximized by carrying out the reaction ________.

Accepted Answer

A) at high temperature and high pressure 
B) at high temperature and low pressure 
C) at low temperature and low pressure 
D) at low temperature and high pressure 
E) in the presence of solid carbon 
A) at high temperature and high pressure 
B) at high temperature and low pressure 
C) at low temperature and low pressure 
D) at low temperature and high pressure 
E) in the presence of solid carbon

Question 10

The value of Keq for the equilibrium H2 (g)+ I2 (g)   2HI (g)
Is 54.0 at 427 °C.What is the value of Keq for the equilibrium below?
HI (g)   1/2 H2 (g)+ 1/2 I2(g)

Accepted Answer

A) 27 
B) 7.35 
C) 0.136 
D) 2.92 × 103 
E) 3.43 × 10-4 
A) 27 
B) 7.35 
C) 0.136 
D) 2.92 × 103 
E) 3.43 × 10-4

Question 11

Given the following reaction at equilibrium at 300.0 K: NH4HS (s)   NH3 (g)+ H2S (g)
If pNH3 = pH2S = 0.105 atm,Kp = ________.

Accepted Answer

A) .0110 
B) 4.99 × 10-4 
C) .105 
D) .0821 
E) 5.66 × 10-3 
A) .0110 
B) 4.99 × 10-4 
C) .105 
D) .0821 
E) 5.66 × 10-3

Question 12

At equilibrium,________.

Accepted Answer

A) all chemical reactions have ceased 
B) the rates of the forward and reverse reactions are equal 
C) the rate constants of the forward and reverse reactions are equal 
D) the value of the equilibrium constant is 1 
E) the limiting reagent has been consumed 
A) all chemical reactions have ceased 
B) the rates of the forward and reverse reactions are equal 
C) the rate constants of the forward and reverse reactions are equal 
D) the value of the equilibrium constant is 1 
E) the limiting reagent has been consumed

Question 13

At 24°C,Kp = 0.080 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) 0.28 
B) 0.080 
C) 0.052 
D) 0.0049 
E) 3.8 
A) 0.28 
B) 0.080 
C) 0.052 
D) 0.0049 
E) 3.8

Question 14

The effect of a catalyst on an equilibrium is to ________.

Accepted Answer

A) increase the rate of the forward reaction only 
B) increase the equilibrium constant so that products are favored 
C) slow the reverse reaction only 
D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture 
E) shift the equilibrium to the right 
A) increase the rate of the forward reaction only 
B) increase the equilibrium constant so that products are favored 
C) slow the reverse reaction only 
D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture 
E) shift the equilibrium to the right

Question 15

= 0.0198 at 721 K for the reaction 2HI (g)     (g)+   (g)
In a particular experiment,the partial pressures of   and   at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm.

Accepted Answer

A) 7.87 
B) 27.0 
C) 5.19 
D) 0.103 
E) 0.0106 
A) 7.87 
B) 27.0 
C) 5.19 
D) 0.103 
E) 0.0106

Question 16

Fritz Haber was awarded the ________ Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen.

Accepted Answer

A) 1954 
B) 1918 
C) 1933 
D) 1900 
E) 1912 
A) 1954 
B) 1918 
C) 1933 
D) 1900 
E) 1912

Question 17

If the value for the equilibrium constant is much less than 1,then the equilibrium mixture contains mostly ________.

Accepted Answer

The answer of If the value for the equilibrium constant...

Question 18

The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g)+ O2 (g)   2NO2 (g)
What is the value of Keq at this temperature for the following reaction?
2NO2 (g)   2NO (g)+ O2 (g)

Accepted Answer

A) 5.4 × 10-13 
B) 1.9 × 10-14 
C) 5.4 × 1013 
D) 5.66 × 10-3 
E) none of the above 
A) 5.4 × 10-13 
B) 1.9 × 10-14 
C) 5.4 × 1013 
D) 5.66 × 10-3 
E) none of the above

Question 19

If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature,________ must be converted to ________ for the system to reach equilibrium.

Accepted Answer

The answer of If the reaction quotient Q for a...

Question 20

In an experiment,0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel to yield CH3OH.At equilibrium,there were 0.29 mol of CO remaining.Keq at the temperature of the experiment is ________.

Accepted Answer

A) 2.80 
B) 17.5 
C) 0.357 
D) 14.5 
E) none of the above 
A) 2.80 
B) 17.5 
C) 0.357 
D) 14.5 
E) none of the above

Exam 15: Chemical Equilibrium

The equilibrium constant for the gas phase reaction 2SO2 (g)+ O2 (g) 2SO3 (g) Is Keq = 2.80 × 102 at 999 K.At equilibrium,________.

Define the reaction quotient.

Le Châtelier's principle states that if a system at equilibrium is disturbed,then more reactants are produced.

Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with of N2O4.At equilibrium at 373 K,0.0055 mol of N2O4 remains.Keq for this reaction is ________.

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

The value of Keq for the equilibrium H2 (g)+ I2 (g) 2HI (g) Is 794 at 25 °C.At this temperature,what is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g)+ 1/2 I2 (g)

The equilibrium constant for the gas phase reaction 2NH3 (g) N2 (g)+ 3H2 (g) Is Keq = 230 at 300 °C.At equilibrium,________.

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g)+ (g) A sample of NOBr (0.64 mol)was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium?

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g)+ O2 (g)ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g)can be maximized by carrying out the reaction ________.

The value of Keq for the equilibrium H2 (g)+ I2 (g) 2HI (g) Is 54.0 at 427 °C.What is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g)+ 1/2 I2(g)

Given the following reaction at equilibrium at 300.0 K: NH4HS (s) NH3 (g)+ H2S (g) If pNH3 = pH2S = 0.105 atm,Kp = ________.

At equilibrium,________.

At 24°C,Kp = 0.080 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.

The effect of a catalyst on an equilibrium is to ________.

= 0.0198 at 721 K for the reaction 2HI (g) (g)+ (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm.

Fritz Haber was awarded the ________ Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen.

If the value for the equilibrium constant is much less than 1,then the equilibrium mixture contains mostly ________.

The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g)+ O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? 2NO2 (g) 2NO (g)+ O2 (g)

If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature,________ must be converted to ________ for the system to reach equilibrium.

In an experiment,0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel to yield CH3OH.At equilibrium,there were 0.29 mol of CO remaining.Keq at the temperature of the experiment is ________.

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

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The equilibrium constant for the gas phase reaction 2SO₂ (g)+ O₂ (g) 2SO₃ (g) Is K_eq = 2.80 × 10² at 999 K.At equilibrium,________.

Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with of N₂O₄.At equilibrium at 373 K,0.0055 mol of N₂O₄ remains.K_eq for this reaction is ________.

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2HI (g) Is 794 at 25 °C.At this temperature,what is the value of K_eq for the equilibrium below? HI (g) 1/2 H₂ (g)+ 1/2 I₂ (g)

The equilibrium constant for the gas phase reaction 2NH₃ (g) N₂ (g)+ 3H₂ (g) Is K_eq = 230 at 300 °C.At equilibrium,________.

Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g)+ O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g)can be maximized by carrying out the reaction ________.

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2HI (g) Is 54.0 at 427 °C.What is the value of K_eq for the equilibrium below? HI (g) 1/2 H₂ (g)+ 1/2 I₂(g)

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g)+ H₂S (g) If pNH₃ = pH₂S = 0.105 atm,K_p = ________.

At 24°C,K_p = 0.080 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.

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g)+ O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? 2NO₂ (g) 2NO (g)+ O₂ (g)

If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature, must be converted to for the system to reach equilibrium.

In an experiment,0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel to yield CH₃OH.At equilibrium,there were 0.29 mol of CO remaining.K_eq at the temperature of the experiment is ________.