Question 1

Which of the following statements is true?

Accepted Answer

A) 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. 
A) 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.

Question 2

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 M 
A) 0.14 M 
B) 0.17 M 
C) 0.27 M 
D) 0.34 M

Question 3

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 M 
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 M

Question 4

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 × 10-2 
A) 2.1 × 10-2 
B) 29 
C) 47 
D) 3.4 × 10-2 
E) 8.7 × 10-2

Question 5

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) 1.13 
A) 2.13 
B) 0.685 
C) 3.11 
D) 1.46 
E) 1.13

Question 6

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. 
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.

Question 7

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 atm 
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 atm

Question 8

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. 
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.

Question 9

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

Question 10

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

Question 11

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) 0.030 
A) 0.020 
B) 43.0 
C) 50.0 
D) 0.030

Question 12

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 M 
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 M

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

Question 14

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 M 
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 M

Question 15

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. 
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.

Question 16

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 M 
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 M

Question 17

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) 0.040 
A) 25 
B) 0.12 
C) 0.99 
D) 8.3 
E) 0.040

Question 18

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 × 104 
A) 2.4 × 10-2 
B) 4.4 × 104 
C) 41 
D) 2.3 × 10-5 
E) 1.9 × 104

Question 19

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

Accepted Answer

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

Question 20

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 M 
A) 7.1 × 10-7 M 
B) 8.4 × 10-4 M 
C) 1.4 × 10-2 M 
D) 1.2 × 10-1 M

Which of the following statements is true?

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?

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

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)

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 = ?

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)

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?

Match the following. -Q = K

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

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

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)

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?

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

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?

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?

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.

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)

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

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?

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Exam 14: Chemical Equilibrium

Which of the following statements is true?

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?

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

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)

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 = ?

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)

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?

Match the following. -Q = K

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

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

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)

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.

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?

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

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?

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?

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.

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)

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

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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Solutions

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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?

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

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)

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 = ?

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)

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?

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

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)

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?

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

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?

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?

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.

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)

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

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?