Question 1

For the equilibrium A2(g)  2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established?

Accepted Answer

A)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) All of the above
G) B) and D)

Question 2

Consider the equilibrium equation C(s) + O2(g)  CO2(g), where ΔHrxn = -393.5 kJ/mol.
The reaction will shift toward the ________ if the temperature of the system is decreased.

Accepted Answer

Question 3

When the following reaction is at equilibrium
2NOCl(g)  2NO(g) + Cl2(g)
then [NO]2 [Cl2] = Kc [NOCl]2.

Accepted Answer

A) True 
 B)False

Question 4

If Q<K then less reactants are observed as the reaction proceeds to ________.

Accepted Answer

The answer of If Q<K then less reactants are observed...

Question 5

The formation constant for the reaction Ag+(aq)  + 2NH3(aq)  +(aq)  + 2NH3(aq)    Ag(NH3) 2+(aq)  Is Kf = 1.7 × 107 at 25°C. What is ΔG° at this temperature? (R = 8.314 J/K• mol)  A)  -1.5 kJ/mol B)  -3.5 kJ/mol C)  -18 kJ/mol D)  -23 kJ/mol E)  -41 kJ/mol" class="answers-bank-image d-inline" rel="preload" > Ag(NH3) 2+(aq) 
Is Kf = 1.7 × 107 at 25°C. What is ΔG° at this temperature? (R = 8.314 J/K• mol)

Accepted Answer

A)   -1.5 kJ/mol
B)   -3.5 kJ/mol
C)   -18 kJ/mol
D)   -23 kJ/mol
E)   -41 kJ/molF) B) and C)
G) A) and B)

Question 6

At 35ºC, the equilibrium constant for the reaction 2NOCl(g)  2(g)  is Kc = 1.6 × 10-5. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10-2 M; [NOCl] = 2.8 × 10-1 M. Calculate the concentration of NO(g)  at equilibrium. A)  1.0 × 10-4 M B)  1.0 × 10-2 M C)  2.8 × 10-1 M D)  2.4 × 10-2 M E)  1.6 × 10-3 M" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + Cl2(g)  is Kc = 1.6 × 10-5. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10-2 M; [NOCl] = 2.8 × 10-1 M. Calculate the concentration of NO(g)  at equilibrium.

Accepted Answer

A)   1.0 × 10-4 M
B)   1.0 × 10-2 M
C)   2.8 × 10-1 M
D)   2.4 × 10-2 M
E)   1.6 × 10-3 MF) A) and B)
G) A) and C)

Question 7

Which substances are included in the equilibrium constant expression, Kc?

Accepted Answer

A)   Only pure solids
B)   Only pure liquids
C)   Only pure solids and liquids
D)   Only gases and dissolved substances
E)   All participating substancesF) B) and E)
G) A) and B)

Question 8

If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as

Accepted Answer

A)   a reversible process.
B)   an elementary process.
C)   at equilibrium.
D)   forbidden.
E)   a forward process.F) B) and C)
G) A) and E)

Question 9

The observation that at equilibrium, the reaction quotient equals the equilibrium constant, is representative of which law?

Accepted Answer

A)   Law of equal states
B)   Reversibility law
C)   Law of equivalence
D)   Law of reactant-product equivalence
E)   Law of mass actionF) A) and D)
G) All of the above

Question 10

The equilibrium constant expression for the reaction
CuO(s) + H2(g)  Cu(s) + H2O(g) is Kc = [H2]/[H2O].

Accepted Answer

A) True 
 B)False

Question 11

Which statement is correct?

Accepted Answer

A)   When Q 
B)   When Q 
C)   When Q = K then ΔG = 0.
D)   When Q > K then ΔG = 1.
E)   When Q > K then ΔG = - RT.F) None of the above
G) A) and E)

Question 12

Suppose 50.0 g of N2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product, N2O4(g)  2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product, N2O4(g)    2NO2(g) . For this reaction Kc = 0.133. Once the system has reached equilibrium, 5.00 g of NO2 is injected into the vessel, and the system is allowed to equilibrate once again. What is the mass of N2O4 in the final equilibrium mixture? A)  39.5 g B)  35.3 g C)  30.3 g D)  25.2 g E)  43.7 g" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) . For this reaction Kc = 0.133. Once the system has reached equilibrium, 5.00 g of NO2 is injected into the vessel, and the system is allowed to equilibrate once again. What is the mass of N2O4 in the final equilibrium mixture?

Accepted Answer

A)   39.5 g
B)   35.3 g
C)   30.3 g
D)   25.2 g
E)   43.7 gF) A) and C)
G) B) and E)

Question 13

Consider this reaction at equilibrium at a total pressure: 2H2O(g)  + O2(g)  2O(g)  + O2(g)    2H2O2(g)  Suppose the volume of this system is twice its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be A)  more than half the total initial pressure. B)  twice the total pressure. C)  less than half the total initial pressure. D)  unchanged. E)  exactly one half of the initial total pressure." class="answers-bank-image d-inline" rel="preload" > 2H2O2(g) 
Suppose the volume of this system is twice its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

Accepted Answer

A)   more than half the total initial pressure.
B)   twice the total pressure.
C)   less than half the total initial pressure.
D)   unchanged.
E)   exactly one half of the initial total pressure.F) A) and B)
G) C) and E)

Question 14

Increasing the temperature of an exothermic reaction causes the equilibrium constant to increase and shifts the equilibrium toward products.

Accepted Answer

A) True 
 B)False

Question 15

Consider the reversible reaction: 2NO2(g)  2(g)    N2O4(g)  If the concentrations of both NO2 and N2O4 are each 0.016 M, what is the value of Qc? A)  0.016 B)  0.50 C)  1.0 D)  2.0 E)  63" class="answers-bank-image d-inline" rel="preload" > N2O4(g)  If the concentrations of both NO2 and N2O4 are each 0.016 M, what is the value of Qc?

Accepted Answer

A)   0.016
B)   0.50
C)   1.0
D)   2.0
E)   63F) A) and E)
G) C) and E)

Question 16

A change in the temperature can change the value of the equilibrium constant.

Accepted Answer

A) True 
 B)False

Question 17

At a certain temperature the reaction CO2(g)  + H2(g)  2(g)  + H2(g)    CO(g)  + H2O(g)  Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.50 mol of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what is the equilibrium concentration of carbon monoxide? A)  0.209 M B)  1.33 M C)  0.267 M D)  0.667 M E)  0.600 M" class="answers-bank-image d-inline" rel="preload" > CO(g)  + H2O(g) 
Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.50 mol of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what is the equilibrium concentration of carbon monoxide?

Accepted Answer

A)   0.209 M
B)   1.33 M
C)   0.267 M
D)   0.667 M
E)   0.600 MF) B) and C)
G) All of the above

Question 18

Consider the chemical reaction 2NH3(g)  N2(g) + 3H2(g). The equilibrium is to be established in a 1.0-L container at 1000 K, where Kc = 4.0 × 10-2. Initially, 1.22 moles of NH3(g) are present. What is the equilibrium concentration of H2(g)?

Accepted Answer

Question 19

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I2 concentration to increase? 2NOI(g)  2 concentration to increase? 2NOI(g)    2NO(g)  + I2(g) , ΔHºrxn = 45.3 kJ/mol A)  Add some NO B)  Expand the gas mixture into a larger volume C)  Decrease the temperature D)  Increase the system pressure E)  Remove some NOI" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + I2(g) , ΔHºrxn = 45.3 kJ/mol

Accepted Answer

A)   Add some NO
B)   Expand the gas mixture into a larger volume
C)   Decrease the temperature
D)   Increase the system pressure
E)   Remove some NOIF) None of the above
G) A) and E)

Question 20

Hydrogen peroxide (H2O2)  decomposes according to the following equation. H2O2(l)  → H2O(l)  + ½O2(g) .
What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol, ΔS° = 70.1 J/K • mol, R = 8.314 J/K • mol)

Accepted Answer

A)   1.3 × 10-21
B)   20.9
C)   3.46 × 1017
D)   7.4 × 1020
E)   8.6 × 104F) B) and D)
G) A) and D)

Exam 15: Chemical Equilibrium

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M, what is the value of Q_c?

Correct Answer
verified

Consider this reaction at equilibrium at a total pressure: 2H₂O(g) + O₂(g) 2H₂O₂(g) Suppose the volume of this system is twice its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

Correct Answer
verified

Which substances are included in the equilibrium constant expression, K_c?

Correct Answer
verified

Consider the equilibrium equation C(s) + O₂(g) CO₂(g), where ΔH_rxn = -393.5 kJ/mol. The reaction will shift toward the ________ if the temperature of the system is decreased.

Correct Answer
verified

If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as

Correct Answer
verified

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.50 mol of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what is the equilibrium concentration of carbon monoxide?

Correct Answer
verified

A change in the temperature can change the value of the equilibrium constant.

Correct Answer
verified

Hydrogen peroxide (H₂O₂) decomposes according to the following equation. H₂O₂(l) → H₂O(l) + ½O₂(g) . What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol, ΔS° = 70.1 J/K • mol, R = 8.314 J/K • mol)

Correct Answer
verified

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) is K_c = 1.6 × 10^-5. An equilibrium mixture was found to have the following concentrations of Cl₂ and NOCl: [Cl₂] = 1.2 × 10^-2^M; [NOCl] = 2.8 × 10^-1^M. Calculate the concentration of NO(g) at equilibrium.

Correct Answer
verified

If Q<K then less reactants are observed as the reaction proceeds to ________.

Correct Answer
verified

The equilibrium constant expression for the reaction CuO(s) + H₂(g) Cu(s) + H₂O(g) is K_c = [H₂]/[H₂O].

Correct Answer
verified

Which statement is correct?

Correct Answer
verified

Increasing the temperature of an exothermic reaction causes the equilibrium constant to increase and shifts the equilibrium toward products.

Correct Answer
verified

For the equilibrium A₂(g) 2A(g) , if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Q_c and time as equilibrium is established?

Correct Answer
verified

When the following reaction is at equilibrium 2NOCl(g) 2NO(g) + Cl₂(g) then [NO]² [Cl₂] = K_c[NOCl]².

Correct Answer
verified

Correct Answer
verified

The formation constant for the reaction Ag⁺(aq) + 2NH₃(aq) Ag(NH₃) ₂⁺(aq) Is K_f = 1.7 × 10⁷ at 25°C. What is ΔG° at this temperature? (R = 8.314 J/K• mol)

Correct Answer
verified

The observation that at equilibrium, the reaction quotient equals the equilibrium constant, is representative of which law?

Correct Answer
verified

Consider the chemical reaction 2NH₃(g) N₂(g) + 3H₂(g). The equilibrium is to be established in a 1.0-L container at 1000 K, where K_c = 4.0 × 10^-2. Initially, 1.22 moles of NH₃(g) are present. What is the equilibrium concentration of H₂(g)?

Correct Answer
verified

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I₂ concentration to increase? 2NOI(g) 2NO(g) + I₂(g) , ΔHº_rxn= 45.3 kJ/mol

Correct Answer
verified

Exam 15: Chemical Equilibrium

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are each 0.016 M, what is the value of Qc?

Correct AnswerverifiedShow Answer

Consider this reaction at equilibrium at a total pressure: 2H2O(g) + O2(g) 2H2O2(g) Suppose the volume of this system is twice its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

Correct AnswerverifiedShow Answer

Which substances are included in the equilibrium constant expression, Kc?

Correct AnswerverifiedShow Answer

Consider the equilibrium equation C(s) + O2(g) CO2(g), where ΔHrxn = -393.5 kJ/mol. The reaction will shift toward the ________ if the temperature of the system is decreased.

Correct AnswerverifiedShow Answer

If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as

Correct AnswerverifiedShow Answer

At a certain temperature the reaction CO2(g) + H2(g) CO(g) + H2O(g) Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.50 mol of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what is the equilibrium concentration of carbon monoxide?

Correct AnswerverifiedShow Answer

A change in the temperature can change the value of the equilibrium constant.

Correct AnswerverifiedShow Answer

Hydrogen peroxide (H2O2) decomposes according to the following equation. H2O2(l) → H2O(l) + ½O2(g) . What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol, ΔS° = 70.1 J/K • mol, R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl2(g) is Kc = 1.6 × 10-5. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10-2 M; [NOCl] = 2.8 × 10-1 M. Calculate the concentration of NO(g) at equilibrium.

Correct AnswerverifiedShow Answer

If Q<K then less reactants are observed as the reaction proceeds to ________.

Correct AnswerverifiedShow Answer

The equilibrium constant expression for the reaction CuO(s) + H2(g) Cu(s) + H2O(g) is Kc = [H2]/[H2O].

Correct AnswerverifiedShow Answer

Which statement is correct?

Correct AnswerverifiedShow Answer

Increasing the temperature of an exothermic reaction causes the equilibrium constant to increase and shifts the equilibrium toward products.

Correct AnswerverifiedShow Answer

For the equilibrium A2(g) 2A(g) , if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Qc and time as equilibrium is established?

Correct AnswerverifiedShow Answer

When the following reaction is at equilibrium 2NOCl(g) 2NO(g) + Cl2(g) then [NO]2 [Cl2] = Kc [NOCl]2.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The formation constant for the reaction Ag+(aq) + 2NH3(aq) Ag(NH3) 2+(aq) Is Kf = 1.7 × 107 at 25°C. What is ΔG° at this temperature? (R = 8.314 J/K• mol)

Correct AnswerverifiedShow Answer

The observation that at equilibrium, the reaction quotient equals the equilibrium constant, is representative of which law?

Correct AnswerverifiedShow Answer

Consider the chemical reaction 2NH3(g) N2(g) + 3H2(g). The equilibrium is to be established in a 1.0-L container at 1000 K, where Kc = 4.0 × 10-2. Initially, 1.22 moles of NH3(g) are present. What is the equilibrium concentration of H2(g)?

Correct AnswerverifiedShow Answer

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I2 concentration to increase? 2NOI(g) 2NO(g) + I2(g) , ΔHºrxn = 45.3 kJ/mol

Correct AnswerverifiedShow Answer

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M, what is the value of Q_c?

Correct Answer
verified

Consider this reaction at equilibrium at a total pressure: 2H₂O(g) + O₂(g) 2H₂O₂(g) Suppose the volume of this system is twice its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

Correct Answer
verified

Which substances are included in the equilibrium constant expression, K_c?

Correct Answer
verified

Consider the equilibrium equation C(s) + O₂(g) CO₂(g), where ΔH_rxn = -393.5 kJ/mol. The reaction will shift toward the ________ if the temperature of the system is decreased.

Correct Answer
verified

Correct Answer
verified

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.50 mol of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what is the equilibrium concentration of carbon monoxide?

Correct Answer
verified

Correct Answer
verified

Hydrogen peroxide (H₂O₂) decomposes according to the following equation. H₂O₂(l) → H₂O(l) + ½O₂(g) . What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol, ΔS° = 70.1 J/K • mol, R = 8.314 J/K • mol)

Correct Answer
verified

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) is K_c = 1.6 × 10^-5. An equilibrium mixture was found to have the following concentrations of Cl₂ and NOCl: [Cl₂] = 1.2 × 10^-2^M; [NOCl] = 2.8 × 10^-1^M. Calculate the concentration of NO(g) at equilibrium.

Correct Answer
verified

Correct Answer
verified

The equilibrium constant expression for the reaction CuO(s) + H₂(g) Cu(s) + H₂O(g) is K_c = [H₂]/[H₂O].

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the equilibrium A₂(g) 2A(g) , if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Q_c and time as equilibrium is established?

Correct Answer
verified

When the following reaction is at equilibrium 2NOCl(g) 2NO(g) + Cl₂(g) then [NO]² [Cl₂] = K_c[NOCl]².

Correct Answer
verified

Correct Answer
verified

The formation constant for the reaction Ag⁺(aq) + 2NH₃(aq) Ag(NH₃) ₂⁺(aq) Is K_f = 1.7 × 10⁷ at 25°C. What is ΔG° at this temperature? (R = 8.314 J/K• mol)

Correct Answer
verified

Correct Answer
verified

Consider the chemical reaction 2NH₃(g) N₂(g) + 3H₂(g). The equilibrium is to be established in a 1.0-L container at 1000 K, where K_c = 4.0 × 10^-2. Initially, 1.22 moles of NH₃(g) are present. What is the equilibrium concentration of H₂(g)?

Correct Answer
verified

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I₂ concentration to increase? 2NOI(g) 2NO(g) + I₂(g) , ΔHº_rxn= 45.3 kJ/mol

Correct Answer
verified