Question 1

Express the equilibrium constant for the following reaction. 3 CH3Cl(g)+ 3/2 Cl2(g)⇔ 3 CH2Cl2(g)+ 3/2 H2(g)

Accepted Answer

A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =   
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =   A

Question 2

Identify the change that will always shift the equilibrium to the right.

Accepted Answer

A)  remove reactant 
B)  increase product 
C)  remove product 
D)  increase pressure 
E)  increase volume 
A)  remove reactant 
B)  increase product 
C)  remove product 
D)  increase pressure 
E)  increase volume C

Question 3

The Kp for the reaction below is 1.49 × 108 at 100.0°C: CO(g)+ Cl2(g)→ COCl2(g)
In an equilibrium mixture of the three gases,PCO =   = 4.44 × 10-4 atm.The partial pressure of the product,phosgene (COCl2),is ________ atm.

Accepted Answer

A)  2.94 × 101 
B)  7.56 × 1014 
C)  1.32 × 10-15 
D)  6.62 × 104 
E)  3.33 × 1011 
A)  2.94 × 101 
B)  7.56 × 1014 
C)  1.32 × 10-15 
D)  6.62 × 104 
E)  3.33 × 1011 A

Question 4

Give the direction of the reaction,if K >> 1.

Accepted Answer

A)  The forward reaction is favored. 
B)  The reverse reaction is favored. 
C)  Neither direction is favored. 
D)  If the temperature is raised, then the forward reaction is favored. 
E)  If the temperature is raised, then the reverse reaction is favored. 
A)  The forward reaction is favored. 
B)  The reverse reaction is favored. 
C)  Neither direction is favored. 
D)  If the temperature is raised, then the forward reaction is favored. 
E)  If the temperature is raised, then the reverse reaction is favored.

Question 5

In a reaction mixture containing reactants and products,each at a concentration of 1M,what is the value of Q?

Accepted Answer

A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations. 
A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations.

Question 6

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g)+ O2(g)⇌ 2 SO3(g).
If initial concentrations are [SO2] = 1.20 M,[O2] = 0.45 M,and [SO3] = 1.80 M,the system is

Accepted Answer

A)  at equilibrium. 
B)  not at equilibrium and will remain in an unequilibrated state. 
C)  not at equilibrium and will shift to the left to achieve an equilibrium state. 
D)  not at equilibrium and will shift to the right to achieve an equilibrium state. 
A)  at equilibrium. 
B)  not at equilibrium and will remain in an unequilibrated state. 
C)  not at equilibrium and will shift to the left to achieve an equilibrium state. 
D)  not at equilibrium and will shift to the right to achieve an equilibrium state.

Question 7

At a certain temperature,nitrogen and hydrogen react to form ammonia: N2(g)+ 3 H2(g)⇌ 2 NH3(g).
When initial amounts of N2,H2,and NH3 are mixed,the concentration of NH3 increases.Which statement below is TRUE?

Accepted Answer

A)  Kc c > Q 
C)  Kc = Q 
D)  More information is needed to make a statement about Kc. 
A)  Kc c > Q 
C)  Kc = Q 
D)  More information is needed to make a statement about Kc.

Question 8

In a reaction mixture containing only products,what is the value of Q?

Accepted Answer

A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations. 
A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations.

Question 9

What is △n for the following equation in relating Kc to Kp?
2 Rb(s)+ 2 H2O(l)⇌ 2 RbOH(aq)+ H2(g)

Accepted Answer

A)  3 
B)  -1 
C)  -2 
D)  2 
E)  1 
A)  3 
B)  -1 
C)  -2 
D)  2 
E)  1

Question 10

The following reaction is exothermic.Which change will shift the equilibrium to the left?
2 SO2(g)+ O2(g)⇌ 2 SO3(g)

Accepted Answer

A)  raising the temperature 
B)  adding SO3 
C)  removing O2 
D)  all of the above 
E)  none of the above 
A)  raising the temperature 
B)  adding SO3 
C)  removing O2 
D)  all of the above 
E)  none of the above

Question 11

Express the equilibrium constant for the following reaction. 2 N2(g)+ 6 H2(g)⇔ 4 NH3(g)

Accepted Answer

A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =   
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =

Question 12

Express the equilibrium constant for the following reaction. 10 NH3(g)⇔ 5 N2(g)+ 15 H2(g)

Accepted Answer

A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =   
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =

Question 13

Chemical equilibrium is the result of

Accepted Answer

A)  all of the reactants being converted into products. 
B)  stoppage of further reaction. 
C)  formation of products equal in mass to the mass of the reactants. 
D)  opposing reactions attaining equal rates. 
E)  a loss of pressure in the system. 
A)  all of the reactants being converted into products. 
B)  stoppage of further reaction. 
C)  formation of products equal in mass to the mass of the reactants. 
D)  opposing reactions attaining equal rates. 
E)  a loss of pressure in the system.

Question 14

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction:
2 CO(g)+ O2(g)⇌ 2 CO2(g).
What is the equilibrium concentration of CO?

Accepted Answer

A)  4.8 × 10-6 M 
B)  2.2 × 10-3 M 
C)  9.3 × 10-2 M 
D)  3.1 × 10-1 M 
A)  4.8 × 10-6 M 
B)  2.2 × 10-3 M 
C)  9.3 × 10-2 M 
D)  3.1 × 10-1 M

Question 15

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g)+ 2B(g)⇌ AB2(g)Kc = 59
AB2(g)+ B(g)⇌ AB3(g)Kc = ?
A(g)+ 3B(g)⇌ AB3(g)Kc = 478

Accepted Answer

A)  3.5 × 10-5 
B)  2.8 × 104 
C)  8.1 
D)  0.12 
E)  89 
A)  3.5 × 10-5 
B)  2.8 × 104 
C)  8.1 
D)  0.12 
E)  89

Question 16

Consider the following reaction: CO2(g)+ C(graphite)⇌ 2 CO(g)
A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

Accepted Answer

A)  0.83 atm 
B)  0.31 atm 
C)  0.26 atm 
D)  0.58 atm 
E)  0.42 atm 
A)  0.83 atm 
B)  0.31 atm 
C)  0.26 atm 
D)  0.58 atm 
E)  0.42 atm

Question 17

Can the Kp and Kc for a reaction ever have the same value?
 Why or why not?

Accepted Answer

Yes,they can have the same value.Since K

Question 18

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g).
If a 3.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

Accepted Answer

A)  0.700 mol 
B)  0.200 mol 
C)  0.107 mol 
D)  0.0114 mol 
A)  0.700 mol 
B)  0.200 mol 
C)  0.107 mol 
D)  0.0114 mol

Question 19

What is Δn for the following equation in relating Kc to Kp?
SO3(g)+ NO(g)⇌ SO2(g)+ NO2(g)

Accepted Answer

A)  0 
B)  -1 
C)  -2 
D)  2 
E)  1 
A)  0 
B)  -1 
C)  -2 
D)  2 
E)  1

Question 20

The reaction below has a Kp value of 41.What is the value of Kc for this reaction at 400 K?
N2(g)+ 3 H2(g)⇌ 2 NH3(g)

Accepted Answer

A)  3.8 × 10-2 
B)  4.4 × 104 
C)  26 
D)  2.3 × 10-5 
E)  41 
A)  3.8 × 10-2 
B)  4.4 × 104 
C)  26 
D)  2.3 × 10-5 
E)  41

Exam 16: Chemical Equilibrium

Express the equilibrium constant for the following reaction. 3 CH3Cl(g)+ 3/2 Cl2(g)⇔ 3 CH2Cl2(g)+ 3/2 H2(g)

Identify the change that will always shift the equilibrium to the right.

The Kp for the reaction below is 1.49 × 108 at 100.0°C: CO(g)+ Cl2(g)→ COCl2(g) In an equilibrium mixture of the three gases,PCO = = 4.44 × 10-4 atm.The partial pressure of the product,phosgene (COCl2),is ________ atm.

Give the direction of the reaction,if K >> 1.

In a reaction mixture containing reactants and products,each at a concentration of 1M,what is the value of Q?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g)+ O2(g)⇌ 2 SO3(g). If initial concentrations are [SO2] = 1.20 M,[O2] = 0.45 M,and [SO3] = 1.80 M,the system is

At a certain temperature,nitrogen and hydrogen react to form ammonia: N2(g)+ 3 H2(g)⇌ 2 NH3(g). When initial amounts of N2,H2,and NH3 are mixed,the concentration of NH3 increases.Which statement below is TRUE?

In a reaction mixture containing only products,what is the value of Q?

What is △n for the following equation in relating Kc to Kp? 2 Rb(s)+ 2 H2O(l)⇌ 2 RbOH(aq)+ H2(g)

The following reaction is exothermic.Which change will shift the equilibrium to the left? 2 SO2(g)+ O2(g)⇌ 2 SO3(g)

Express the equilibrium constant for the following reaction. 2 N2(g)+ 6 H2(g)⇔ 4 NH3(g)

Express the equilibrium constant for the following reaction. 10 NH3(g)⇔ 5 N2(g)+ 15 H2(g)

Chemical equilibrium is the result of

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). What is the equilibrium concentration of CO?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g)+ 2B(g)⇌ AB2(g)Kc = 59 AB2(g)+ B(g)⇌ AB3(g)Kc = ? A(g)+ 3B(g)⇌ AB3(g)Kc = 478

Consider the following reaction: CO2(g)+ C(graphite)⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). If a 3.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

What is Δn for the following equation in relating Kc to Kp? SO3(g)+ NO(g)⇌ SO2(g)+ NO2(g)

The reaction below has a Kp value of 41.What is the value of Kc for this reaction at 400 K? N2(g)+ 3 H2(g)⇌ 2 NH3(g)

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

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Express the equilibrium constant for the following reaction. 3 CH₃Cl(g)+ 3/2 Cl₂(g)⇔ 3 CH₂Cl₂(g)+ 3/2 H_2(g)

The K_p for the reaction below is 1.49 × 10⁸ at 100.0°C: CO(g)+ Cl₂(g)→ COCl₂(g) In an equilibrium mixture of the three gases,P_CO = = 4.44 × 10^-4 atm.The partial pressure of the product,phosgene (COCl₂),is ________ atm.

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 1.20 M,[O₂] = 0.45 M,and [SO₃] = 1.80 M,the system is

At a certain temperature,nitrogen and hydrogen react to form ammonia: N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g). When initial amounts of N₂,H₂,and NH₃ are mixed,the concentration of NH₃ increases.Which statement below is TRUE?

What is △n for the following equation in relating K_c to K_p? 2 Rb(s)+ 2 H₂O(l)⇌ 2 RbOH(aq)+ H₂(g)

The following reaction is exothermic.Which change will shift the equilibrium to the left? 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

Express the equilibrium constant for the following reaction. 2 N₂(g)+ 6 H₂(g)⇔ 4 NH₃(g)

Express the equilibrium constant for the following reaction. 10 NH₃(g)⇔ 5 N₂(g)+ 15 H₂(g)

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g)+ 2B(g)⇌ AB₂(g)Kc = 59 AB₂(g)+ B(g)⇌ AB₃(g)K_c = ? A(g)+ 3B(g)⇌ AB₃(g)K_c = 478

Consider the following reaction: CO₂(g)+ C(graphite)⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO₂ and 0.32 atm CO.Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25.

Can the K_p and K_c for a reaction ever have the same value? Why or why not?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 3.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

What is Δn for the following equation in relating K_c to K_p? SO₃(g)+ NO(g)⇌ SO₂(g)+ NO₂(g)

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)