Question 1

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO2(g) . 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 108
[SO3]eq = 0.0034 M [O2]eq = 0.0018 M

Accepted Answer

A)   2.8 × 1013 M
B)   1.88 M
C)   6.1 × 10-6 M
D)   1.0 × 103 M
E)   1.4 MF) C) and D)
G) A) and E)

Question 2

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M,[HI]eq = 5.6 × 10-16 M,[Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

Accepted Answer

A)   8.2 × 10-18
B)   2.8 × 1031
C)   1.2 × 1017
D)   1.4 × 10-19
E)   3.5 × 10-32F) All of the above
G) None of the above

Question 3

Match between columns Premises: K << 1 Q < K Q > K Q = K Q >> 1 K ≈ 1

Accepted Answer

The Answer of reaction does not strongly favor reactants or is...

Question 4

Consider the following reaction: COCl2(g) ⇌ CO(g) + Cl2(g) 
A reaction mixture initially contains 1.6 M COCl2.Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4.Calculate this based on the assumption that the answer is negligible compared to 1.6.

Accepted Answer

A)   4.2 × 10-4 M
B)   1.5 × 10-3 M
C)   3.7 × 10-2 M
D)   2.1 × 10-2 M
E)   1.3 × 10-3 MF) B) and E)
G) All of the above

Question 5

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

Accepted Answer

A)   1
B)   3
C)   -2
D)   0
E)   -4F) B) and C)
G) A) and B)

Question 6

Consider the following reaction at equilibrium.What will happen if O2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

Accepted Answer

A)   The equilibrium constant will increase.
B)   The equilibrium will change in the direction of the reactants.
C)   The equilibrium will change in the direction of the products.
D)   No change in equilibrium is observed.
E)   The equilibrium constant will decrease.F) None of the above
G) A) and E)

Question 7

Identify the change that will always shift the equilibrium to the right. 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

Accepted Answer

A)   remove the reactant
B)   adding He
C)   increase the reactant
D)   increase the volume
E)   add CuF) A) and C)
G) A) and E)

Question 8

At 900.0 K,the equilibrium constant (Kp) for the following reaction is 0.345. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) 
At equilibrium,the partial pressure of SO2 is 35.0 atm and that of p) for the following reaction is 0.345. 2 SO2(g) + O2(g) ⇌ 2 SO3(g)  At equilibrium,the partial pressure of SO2 is 35.0 atm and that of   is 15.9 atm.The partial pressure of SO3 is ________ atm. A)  82.0 B)  4.21 ×   C)  192 D)  6.20 × 10-4 E)  40.2" class="answers-bank-image d-inline" rel="preload" > is 15.9 atm.The partial pressure of SO3 is ________ atm.

Accepted Answer

A)   82.0
B)   4.21 × p) for the following reaction is 0.345. 2 SO2(g) + O2(g) ⇌ 2 SO3(g)  At equilibrium,the partial pressure of SO2 is 35.0 atm and that of   is 15.9 atm.The partial pressure of SO3 is ________ atm. 
A)   82.0 
B)   4.21 ×   
C)   192 
D)   6.20 × 10-4 
E)   40.2" class="answers-bank-image d-inline" rel="preload" >
C)   192
D)   6.20 × 10-4
E)   40.2F) B) and C)
G) C) and D)

Question 9

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] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 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.E) A) and B)
F) A) and D)

Question 10

For which reaction will Kp = Kc?

Accepted Answer

A)   C(s)  + O2(g)  ⇌ CO2(g) 
B)   2 HgO(s)  ⇌ Hg(l)  + O2(g) 
C)   CaCO3(s)  ⇌ CaO(s)  + CO2(g) 
D)   H2CO3(s)  ⇌ H2O(l)  + CO2(g) 
E)   2 H2O(l)  ⇌ 2 H2(g)  + O2(g) F) A) and E)
G) A) and D)

Question 11

Express the reverse equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

Accepted Answer

A)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
B)   K =   3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
C)   K =   3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
D)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
E)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >F) B) and C)
G) B) and D)

Question 12

Consider the following reaction at equilibrium.What will happen if SO2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

Accepted Answer

A)   The equilibrium constant will increase.
B)   The equilibrium will change in the direction of the reactants.
C)   The equilibrium will change in the direction of the products.
D)   No change in equilibrium is observed.
E)   The equilibrium constant will decrease.F) C) and D)
G) A) and B)

Question 13

The decomposition of ammonia is: 2 NH3(g) ⇌ N2(g) + 3 H2(g) .If Kp is 1.5 × 103 at 400°C,what is the partial pressure of ammonia at equilibrium when N2 is 0.10 atm and H2 is 0.15 atm?

Accepted Answer

A)   2.2 × 10-7 atm
B)   4.7 × 10-4 atm
C)   2.1 × 103 atm
D)   4.4 × 106 atmE) B) and C)
F) B) and D)

Question 14

Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10
A reaction mixture contains 0.20 M CH4,0.70 M CO2 and 1.5 M H2O.Which of the following statements is TRUE concerning this system?

Accepted Answer

A)   The reaction will shift in the direction of products.
B)   The equilibrium constant will increase.
C)   The reaction quotient will increase.
D)   The reaction will shift in the direction of reactants.
E)   The system is at equilibrium.F) A) and D)
G) C) and D)

Question 15

Why aren't solids or liquids included in an equilibrium expression?

Accepted Answer

The equilibrium constant relates differe...

Question 16

Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation: C6H12 ⇌ MCP
If Kc = 0.143 at 25°C for this reaction,predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.400 M and 0.300 M,respectively.The system

Accepted Answer

A)   will shift left.
B)   will shift right.
C)   is already at equilibrium.
D)   is not at equilibrium and will remain in an unequilibrated state.E) A) and B)
F) A) and C)

Question 17

Which of the following statements is TRUE?

Accepted Answer

A)   If Q 
B)   If Q > K, it means the forward reaction will proceed to form more products.
C)   If Q = K, it means the reaction is at equilibrium.
D)   All of the above are true.
E)   None of the above are true.F) B) and D)
G) A) and E)

Question 18

Define Le Chatelier's Principle.

Accepted Answer

A)   When a chemical system at equilibrium is disturbed, the system shifts in a direction that maximizes the disturbance.
B)   A system will always change if the pressure changes.
C)   When a chemical system at equilibrium is disturbed, the system shifts in a direction that equals the disturbance.
D)   When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance.
E)   A system will always change if the volume changes.F) None of the above
G) A) and B)

Question 19

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F2(g) ⇌ XeF4(g)

Accepted Answer

A)   The reaction will shift to the left in the direction of reactants.
B)   The equilibrium constant will increase.
C)   No effect will be observed.
D)   The reaction will shift to the right in the direction of products.
E)   The equilibrium constant will decrease.F) A) and E)
G) A) and B)

Question 20

Consider the following reaction: Xe(g) + 2 F2(g) ⇌ XeF4(g) 
A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp) for the reaction.

Accepted Answer

A)   25
B)   0.12
C)   0.99
D)   8.3
E)   0.040F) A) and D)
G) C) and D)

Exam 15: Chemical Equilibrium

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 M,[HI]_eq = 5.6 × 10^-16 M,[Cl₂]_eq = 0.0019 M. 2 HCl(g) + I₂(s) ⇌ 2 HI(g) + Cl₂(g)

Correct Answer
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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₂(g) . 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) K_c = 1.7 × 10⁸ [SO₃]_eq = 0.0034 M [O₂]_eq = 0.0018 M

Correct Answer
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Match the following.

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

Correct Answer
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Correct Answer
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Correct Answer
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Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F₂(g) ⇌ XeF₄(g)

Correct Answer
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Why aren't solids or liquids included in an equilibrium expression?

Correct Answer
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The equilibrium constant relates differe...
View Answer

At 900.0 K,the equilibrium constant (K_p) for the following reaction is 0.345. 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) At equilibrium,the partial pressure of SO₂ is 35.0 atm and that of is 15.9 atm.The partial pressure of SO₃ is ________ atm.

Correct Answer
verified

Consider the following reaction: Xe(g) + 2 F₂(g) ⇌ XeF₄(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F₂.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (K_p) for the reaction.

Correct Answer
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Which of the following statements is TRUE?

Correct Answer
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Consider the following reaction at equilibrium.What will happen if SO₂ is added to the reaction? 4 FeS₂(s) + 11 O₂(g) ⇌ 2 Fe₂O₃(s) + 8 SO₂(g)

Correct Answer
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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] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

Correct Answer
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Define Le Chatelier's Principle.

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The decomposition of ammonia is: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.10 atm and H₂ is 0.15 atm?

Correct Answer
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Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH₄(g) ⇌ CO₂(g) + 4 Cu(s) + 2 H₂O(g) K_c = 1.10 A reaction mixture contains 0.20 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

Correct Answer
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For which reaction will K_p = K_c?

Correct Answer
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Consider the following reaction at equilibrium.What will happen if O₂ is added to the reaction? 4 FeS₂(s) + 11 O₂(g) ⇌ 2 Fe₂O₃(s) + 8 SO₂(g)

Correct Answer
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Express the reverse equilibrium constant for the following reaction. 4 CH₃Cl(g) + 2 Cl₂(g) ⇔ 4 CH₂Cl₂(g) + 2 H₂(g)

Correct Answer
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Identify the change that will always shift the equilibrium to the right. 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

Correct Answer
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Exam 15: Chemical Equilibrium

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M,[HI]eq = 5.6 × 10-16 M,[Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO2(g) . 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 108 [SO3]eq = 0.0034 M [O2]eq = 0.0018 M

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Match the following.

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F2(g) ⇌ XeF4(g)

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Why aren't solids or liquids included in an equilibrium expression?

Correct AnswerverifiedThe equilibrium constant relates differe...View AnswerShow Answer

At 900.0 K,the equilibrium constant (Kp) for the following reaction is 0.345. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) At equilibrium,the partial pressure of SO2 is 35.0 atm and that of is 15.9 atm.The partial pressure of SO3 is ________ atm.

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Consider the following reaction: Xe(g) + 2 F2(g) ⇌ XeF4(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp) for the reaction.

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Which of the following statements is TRUE?

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Consider the following reaction at equilibrium.What will happen if SO2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

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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] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

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Define Le Chatelier's Principle.

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The decomposition of ammonia is: 2 NH3(g) ⇌ N2(g) + 3 H2(g) .If Kp is 1.5 × 103 at 400°C,what is the partial pressure of ammonia at equilibrium when N2 is 0.10 atm and H2 is 0.15 atm?

Correct AnswerverifiedShow Answer

Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10 A reaction mixture contains 0.20 M CH4,0.70 M CO2 and 1.5 M H2O.Which of the following statements is TRUE concerning this system?

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For which reaction will Kp = Kc?

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Consider the following reaction at equilibrium.What will happen if O2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

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Express the reverse equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

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Identify the change that will always shift the equilibrium to the right. 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

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Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 M,[HI]_eq = 5.6 × 10^-16 M,[Cl₂]_eq = 0.0019 M. 2 HCl(g) + I₂(s) ⇌ 2 HI(g) + Cl₂(g)

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₂(g) . 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) K_c = 1.7 × 10⁸ [SO₃]_eq = 0.0034 M [O₂]_eq = 0.0018 M

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

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Correct Answer
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Correct Answer
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Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F₂(g) ⇌ XeF₄(g)

Correct Answer
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Correct Answer
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The equilibrium constant relates differe...
View Answer

At 900.0 K,the equilibrium constant (K_p) for the following reaction is 0.345. 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) At equilibrium,the partial pressure of SO₂ is 35.0 atm and that of is 15.9 atm.The partial pressure of SO₃ is ________ atm.

Correct Answer
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Consider the following reaction: Xe(g) + 2 F₂(g) ⇌ XeF₄(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F₂.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (K_p) for the reaction.

Correct Answer
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Correct Answer
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Consider the following reaction at equilibrium.What will happen if SO₂ is added to the reaction? 4 FeS₂(s) + 11 O₂(g) ⇌ 2 Fe₂O₃(s) + 8 SO₂(g)

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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] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

Correct Answer
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Correct Answer
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The decomposition of ammonia is: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.10 atm and H₂ is 0.15 atm?

Correct Answer
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Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH₄(g) ⇌ CO₂(g) + 4 Cu(s) + 2 H₂O(g) K_c = 1.10 A reaction mixture contains 0.20 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

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For which reaction will K_p = K_c?

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Consider the following reaction at equilibrium.What will happen if O₂ is added to the reaction? 4 FeS₂(s) + 11 O₂(g) ⇌ 2 Fe₂O₃(s) + 8 SO₂(g)

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Express the reverse equilibrium constant for the following reaction. 4 CH₃Cl(g) + 2 Cl₂(g) ⇔ 4 CH₂Cl₂(g) + 2 H₂(g)

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Identify the change that will always shift the equilibrium to the right. 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

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