Question 1

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 2

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. 
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.

Question 3

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. 
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.

Question 4

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 5

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.

Accepted Answer

A)  82.0 
B)  4.21 ×   
C)  192 
D)  6.20 × 10-4 
E)  40.2 
A)  82.0 
B)  4.21 ×   
C)  192 
D)  6.20 × 10-4 
E)  40.2

Question 6

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 Cu 
A)  remove the reactant 
B)  adding He 
C)  increase the reactant 
D)  increase the volume 
E)  add Cu

Question 7

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) 
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)

Question 8

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

Question 9

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

Accepted Answer

The equilibrium constant relates differe

Question 10

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. 
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.

Question 11

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 × 10-32 
A)  8.2 × 10-18 
B)  2.8 × 1031 
C)  1.2 × 1017 
D)  1.4 × 10-19 
E)  3.5 × 10-32

Question 12

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. 
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.

Question 13

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 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 14

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

Question 15

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. 
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.

Question 16

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. 
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.

Question 17

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

Question 18

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. 
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 19

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

Exam 15: Chemical Equilibrium

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)

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)

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?

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.

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

For which reaction will Kp = Kc?

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

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

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?

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)

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.

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

Define Le Chatelier's Principle.

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)

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

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

Which of the following statements is TRUE?

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

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)

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?

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.

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

For which reaction will K_p = K_c?

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

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?

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)

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)

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)

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

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

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.