Question 1

Suppose 75.0 g of PCl5(g)  is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) , and the system is allowed to reach equilibrium at 250ºC. PCl5(g)  5(g)  is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) , and the system is allowed to reach equilibrium at 250ºC. PCl5(g)    PCl3(g)  + Cl2(g)  If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.08206 L • atm/K • mol)  A)  6.83 atm B)  8.86 atm C)  5.38 atm D)  3.47 atm E)  1.68atm" class="answers-bank-image d-inline" rel="preload" > PCl3(g)  + Cl2(g) 
If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium?
(R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   6.83 atm
B)   8.86 atm
C)   5.38 atm
D)   3.47 atm
E)   1.68atmF) A) and C)
G) B) and E)

Question 2

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is Kc for this reaction? CO(g)  + Br2(g)  2 was 0.233 M. What is Kc for this reaction? CO(g)  + Br2(g)    COBr2(g)  A)  5.23 B)  2.14 C)  1.17 D)  0.467 E)  0.191" class="answers-bank-image d-inline" rel="preload" > COBr2(g)

Accepted Answer

A)   5.23
B)   2.14
C)   1.17
D)   0.467
E)   0.191F) A) and B)
G) A) and D)

Question 3

At 1500°C the equilibrium constant for the reaction CO(g)  + 2H2(g)  2(g)    CH3OH(g)  has the value KP = 1.4 × 10-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)  A)  105 kJ/mol B)  1.07 kJ/mol C)  -233 kJ/mol D)  -105 kJ/mol E)  233 kJ/mol" class="answers-bank-image d-inline" rel="preload" > CH3OH(g)  has the value KP = 1.4 × 10-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

Accepted Answer

A)   105 kJ/mol
B)   1.07 kJ/mol
C)   -233 kJ/mol
D)   -105 kJ/mol
E)   233 kJ/molF) C) and E)
G) B) and C)

Question 4

Nitrogen dioxide decomposes according to the reaction 2NO2(g)  2(g)    2NO(g)  + O2(g)  Where KP = 4.48 × 10-13 at 25°C. What is the value for Kc?(R = 0.08206 L • atm/K • mol)  A)  1.83 × 10-14 B)  4.48 × 10-14 C)  9.19 × 10-13 D)  2.18 × 10-13 E)  1.10 × 10-11" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + O2(g) 
Where KP = 4.48 × 10-13 at 25°C. What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   1.83 × 10-14
B)   4.48 × 10-14
C)   9.19 × 10-13
D)   2.18 × 10-13
E)   1.10 × 10-11F) A) and B)
G) C) and D)

Question 5

What is the expression for KP for the following reaction? A(g)  P for the following reaction? A(g)    B(g)  + 2C(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > B(g)  + 2C(g)

Accepted Answer

A)   P for the following reaction? A(g)    B(g)  + 2C(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   P for the following reaction? A(g)    B(g)  + 2C(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   P for the following reaction? A(g)    B(g)  + 2C(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   P for the following reaction? A(g)    B(g)  + 2C(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   P for the following reaction? A(g)    B(g)  + 2C(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) C) and E)

Question 6

Which statement is correct?

Accepted Answer

A)   If K 
B)   If K > 1, lnK is negative, and ΔG° is positive, then the reaction is product favored.
C)   If K > 1, lnK is positive, and ΔG° is negative, then the reaction is product favored.
D)   If K > 1, lnK is negative, and ΔG° is negative, then the reaction is reactant favored.
E)   If K < 1, lnK is positive, and ΔG° is positive, then the reaction is reactant favored.F) A) and D)
G) C) and D)

Exam 15: Chemical Equilibrium

Correct Answer
verified

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C. What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Which statement is correct?

Correct Answer
verified

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂ was 0.233 M. What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Correct Answer
verified

At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) CH₃OH(g) has the value K_P = 1.4 × 10^-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

Correct Answer
verified

What is the expression for K_P for the following reaction? A(g) B(g) + 2C(g)

Correct Answer
verified

Exam 15: Chemical Equilibrium

Correct AnswerverifiedShow Answer

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g) Where KP = 4.48 × 10-13 at 25°C. What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Which statement is correct?

Correct AnswerverifiedShow Answer

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is Kc for this reaction? CO(g) + Br2(g) COBr2(g)

Correct AnswerverifiedShow Answer

At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) CH3OH(g) has the value KP = 1.4 × 10-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

What is the expression for KP for the following reaction? A(g) B(g) + 2C(g)

Correct AnswerverifiedShow Answer

Correct Answer
verified

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C. What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Correct Answer
verified

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂ was 0.233 M. What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Correct Answer
verified

At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) CH₃OH(g) has the value K_P = 1.4 × 10^-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

Correct Answer
verified

What is the expression for K_P for the following reaction? A(g) B(g) + 2C(g)

Correct Answer
verified