Question 1

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g) .
NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) Kc = 1.58 × 10-8
[NH3]eq = 2.9 × 10-3 M

Accepted Answer

A)  0.053 M
B)  4.6 × 10-11 M
C)  1.9 × 10-3 M
D)  5.4 × 10-6 M
E)  0.022 MF) D) and E)
G) None of the above

Question 2

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 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)  7.1 × 10-7 M
B)  8.4 × 10-4 M
C)  1.4 × 10-2 M
D)  1.2 × 10-1 ME) B) and C)
F) A) and B)

Question 3

Consider the following reaction:
COCl2(g) ⇌ CO(g) + Cl2(g0
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) A) and E)
G) B) and C)

Question 4

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

Accepted Answer

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

Question 5

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:
PCl5(g) ⇌ PCl3(g) + Cl2(g) 
At 250°C,0.125 M PCl5 is added to the flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

Accepted Answer

A)  [PCl5] = 0.00765 M,[PCl3] = 0.117 M,and [Cl2] = 0.117 M
B)  [PCl5] = 0.0625 M,[PCl3] = 0.335 M,and [Cl2] = 0.335 M
C)  [PCl5] = 1.80 M,[PCl3] = 1.80 M,and [Cl2] = 1.80 M
D)  [PCl5] = 3.96 M,[PCl3] = 3.83 M,and [Cl2] = 3.83 ME) A) and D)
F) A) and C)

Question 6

Express the equilibrium constant for the following reaction.
PCl5(g) ⇌ PCl3(g) + Cl2(g)

Accepted Answer

A)  K = 5(g) ⇌ PCl3(g) + Cl2(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
B)  K = 5(g) ⇌ PCl3(g) + Cl2(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
C)  K = 5(g) ⇌ PCl3(g) + Cl2(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
D)  K = 5(g) ⇌ PCl3(g) + Cl2(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
E)  K = 5(g) ⇌ PCl3(g) + Cl2(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) All of the above

Question 7

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) All of the above
F) A) and D)

Question 8

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) B) and E)
G) A) and E)

Question 9

Match the following.
-Q = K

Accepted Answer

A)  Reaction will favor formation of reactants.
B)  Reaction does not strongly favor reactants or products.
C)  Reaction favors formation of more products.
D)  Reaction has a larger amount of products than reactants.
E)  Reaction is at equilibrium.F) A) and B)
G) A) and C)

Question 10

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g) .
NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) Kc = 1.58 × 10-8
[NH3]eq = 2.3 × 10-3 M

Accepted Answer

A)  0.053 M
B)  3.6 × 10-11 M
C)  3.0 × 10-3 M
D)  6.9 × 10-6 M
E)  0.022 MF) A) and E)
G) B) and E)

Question 11

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
N2O4(g) ⇌ 2 NO2(g) Kc = 1.46
3 N2O4(g) ⇌ 6 NO2(g) Kc = ?

Accepted Answer

A)  2.13
B)  0.685
C)  3.11
D)  1.46
E)  1.13F) A) and E)
G) B) and E)

Question 12

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) All of the above

Question 13

What is the equilibrium constant (Kc) for the reaction
H2(g) + I2(g) ⇌ 2HI(g)  
(Equilibrium concentrations are: [HI] = 1.17 M;[H2] = 0.165 M;[I2] = 0.165 M)

Accepted Answer

A)  0.020
B)  43.0
C)  50.0
D)  0.030E) A) and B)
F) C) and D)

Question 14

The equilibrium constant (Kc) for the reaction N2O4(g) ⇌ 2 NO2 (g) is 5.85 × 10-3 at 10°C.A reaction mixture has 0.025 M of N2O4 and 0.033 M of NO2 at time t.What statement is correct for this reaction at time t?

Accepted Answer

A)  The reaction goes to the left.
B)  The reaction is in equilibrium.
C)  The reaction goes to the right.
D)  The reaction is very slow.E) A) and D)
F) B) and D)

Question 15

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction:
Cis-2-butene ⇌ trans-2-butene.
If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

A)  P(cis-2-butene) = 0.0426 atm and P(trans-2-butene) = 0.145 atm
B)  P(cis-2-butene) = 0.0471 atm and P(trans-2-butene) = 0.160 atm
C)  P(cis-2-butene) = 0.0735 atm and P(trans-2-butene) = 0.250 atm
D)  P(cis-2-butene) = 0.0898 atm and P(trans-2-butene) = 0.305 atmE) B) and D)
F) All of the above

Question 16

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H2.
D2(g) + H2(g) ⇌ 2 HD(g) Kp = 1.80
P(D2) eq = 1.1 × 10-3 atm P(HD) eq = 2.7 × 10-3 atm

Accepted Answer

A)  2.7 atm
B)  1.4 atm
C)  0.73 atm
D)  3.7 × 10-3 atm
E)  8.1 × 10-4 atmF) B) and E)
G) C) and D)

Question 17

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system?
2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

Accepted Answer

A)  The reaction will shift to the right in the direction of products.
B)  No effect will be observed.
C)  The reaction will shift to the left in the direction of reactants.
D)  The equilibrium constant will decrease.
E)  The equilibrium constant will increase.F) A) and E)
G) None of the above

Question 18

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction:
2 ICl(g) ⇌ I2(g) + Cl2(g) .
What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

Accepted Answer

A)  0.14 M
B)  0.17 M
C)  0.27 M
D)  0.34 ME) B) and D)
F) C) and D)

Question 19

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[I2]eq = 0.39 M,[HI]eq = 1.6 M.
H2(g) + I2(g) ⇌ 2 HI(g)

Accepted Answer

A)  2.1 × 10-2
B)  29
C)  47
D)  3.4 × 10-2
E)  8.7 × 10-2F) None of the above
G) C) and E)

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)  2.4 × 10-2
B)  4.4 × 104
C)  41
D)  2.3 × 10-5
E)  1.9 × 104F) None of the above
G) A) and E)

Exam 14: Chemical Equilibrium

Match the following. -Q = K

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
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H₂. D₂(g) + H₂(g) ⇌ 2 HD(g) K_p = 1.80 P(D₂) _eq = 1.1 × 10^-3atm P(HD) _eq = 2.7 × 10^-3 atm

Correct Answer
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g) + I₂(g) ⇌ 2 HI(g)

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
verified

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 1.46 3 N₂O₄(g) ⇌ 6 NO₂(g) K_c = ?

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Correct Answer
verified

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 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?

Correct Answer
verified

What is the equilibrium constant (K_c) for the reaction H₂(g) + I₂(g) ⇌ 2HI(g) (Equilibrium concentrations are: [HI] = 1.17 M;[H₂] = 0.165 M;[I₂] = 0.165 M)

Correct Answer
verified

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0-L flask?

Correct Answer
verified

Express the equilibrium constant for the following reaction. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

Correct Answer
verified

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)

Correct Answer
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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.9 × 10^-3 M

Correct Answer
verified

The equilibrium constant (Kc) for the reaction N₂O₄(g) ⇌ 2 NO₂ (g) is 5.85 × 10^-3at 10°C.A reaction mixture has 0.025 M of N₂O₄and 0.033 M of NO₂at time t.What statement is correct for this reaction at time t?

Correct Answer
verified

Which of the following statements is true?

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H₂S(g) + 3 O₂(g) ⇌ 2 H₂O(g) + 2 SO₂(g)

Correct Answer
verified

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250°C,0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Correct Answer
verified

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

Correct Answer
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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.3 × 10^-3 M

Correct Answer
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Exam 14: Chemical Equilibrium

Match the following. -Q = K

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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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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H2. D2(g) + H2(g) ⇌ 2 HD(g) Kp = 1.80 P(D2) eq = 1.1 × 10-3 atm P(HD) eq = 2.7 × 10-3 atm

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Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[I2]eq = 0.39 M,[HI]eq = 1.6 M. H2(g) + I2(g) ⇌ 2 HI(g)

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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?

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The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2 NO2(g) Kc = 1.46 3 N2O4(g) ⇌ 6 NO2(g) Kc = ?

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The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 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?

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What is the equilibrium constant (Kc) for the reaction H2(g) + I2(g) ⇌ 2HI(g) (Equilibrium concentrations are: [HI] = 1.17 M;[H2] = 0.165 M;[I2] = 0.165 M)

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At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g) . What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

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Express the equilibrium constant for the following reaction. PCl5(g) ⇌ PCl3(g) + Cl2(g)

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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)

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g) . NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) Kc = 1.58 × 10-8 [NH3]eq = 2.9 × 10-3 M

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The equilibrium constant (Kc) for the reaction N2O4(g) ⇌ 2 NO2 (g) is 5.85 × 10-3 at 10°C.A reaction mixture has 0.025 M of N2O4 and 0.033 M of NO2 at time t.What statement is correct for this reaction at time t?

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Which of the following statements is true?

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Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

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Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250°C,0.125 M PCl5 is added to the flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

Correct AnswerverifiedShow Answer

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

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g) . NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) Kc = 1.58 × 10-8 [NH3]eq = 2.3 × 10-3 M

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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
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H₂. D₂(g) + H₂(g) ⇌ 2 HD(g) K_p = 1.80 P(D₂) _eq = 1.1 × 10^-3atm P(HD) _eq = 2.7 × 10^-3 atm

Correct Answer
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g) + I₂(g) ⇌ 2 HI(g)

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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
verified

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 1.46 3 N₂O₄(g) ⇌ 6 NO₂(g) K_c = ?

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Correct Answer
verified

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 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?

Correct Answer
verified

What is the equilibrium constant (K_c) for the reaction H₂(g) + I₂(g) ⇌ 2HI(g) (Equilibrium concentrations are: [HI] = 1.17 M;[H₂] = 0.165 M;[I₂] = 0.165 M)

Correct Answer
verified

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0-L flask?

Correct Answer
verified

Express the equilibrium constant for the following reaction. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

Correct Answer
verified

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)

Correct Answer
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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.9 × 10^-3 M

Correct Answer
verified

The equilibrium constant (Kc) for the reaction N₂O₄(g) ⇌ 2 NO₂ (g) is 5.85 × 10^-3at 10°C.A reaction mixture has 0.025 M of N₂O₄and 0.033 M of NO₂at time t.What statement is correct for this reaction at time t?

Correct Answer
verified

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H₂S(g) + 3 O₂(g) ⇌ 2 H₂O(g) + 2 SO₂(g)

Correct Answer
verified

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250°C,0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Correct Answer
verified

Correct Answer
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.3 × 10^-3 M

Correct Answer
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