Question 1

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III)  oxalate complex ion: Fe3+(aq)  + 3C2O42-(aq)  ⇌ [Fe(C2O4) 3]3-(aq) 
If 0. 0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

Accepted Answer

A)   1.44 × 10-22 mol L-1
B)   0.0100 mol L-1
C)   8.35 × 1019 mol L-1
D)   6.94 × 1021 mol L-1

Question 2

For the following reaction, what is Δn required in the conversion of Kc to Kp? CH4(g)  + H2O(g)  ⇌ CO(g)  + 3H2(g)

Accepted Answer

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

Question 3

Express the equilibrium constant for the following reaction: SO2(g)  + H2O(l)  ⇌ H2SO3(aq)

Accepted Answer

A)   K = 2(g)  + H2O(l)  ⇌ H2SO3(aq)  
A)   K =   
B)   K =   
C)   K =   
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
B)   K = 2(g)  + H2O(l)  ⇌ H2SO3(aq)  
A)   K =   
B)   K =   
C)   K =   
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
C)   K = 2(g)  + H2O(l)  ⇌ H2SO3(aq)  
A)   K =   
B)   K =   
C)   K =   
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
D)   K = 2(g)  + H2O(l)  ⇌ H2SO3(aq)  
A)   K =   
B)   K =   
C)   K =   
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
E)   K = 2(g)  + H2O(l)  ⇌ H2SO3(aq)  
A)   K =   
B)   K =   
C)   K =   
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >

Question 4

Consider the following reaction: 2H2O(g)  + 2SO2(g)  ⇌ 2H2S(g)  + 3O2(g) 
A reaction mixture initially contains 2.8 mol L-1 H2O and 2.6 mol L-1 SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Accepted Answer

A)   0.045 mol L-1
B)   0.058 mol L-1
C)   0.028 mol L-1
D)   3.1 × 10-3 mol L-1
E)   0.12 mol L-1

Question 5

For which of the following reactions will Kc = Kp?

Accepted Answer

A)   H2(g)  + I2(g)  ⇌ 2HI(g) 
B)   CH4(g)  + H2O(g)  ⇌ CO(g)  + 3H2(g) 
C)   N2O4(g)  ⇌ 2NO2(g) 
D)   CO(g)  + 2H2(g)  ⇌ CH3OH(g) 
E)   N2(g)  + 3H2(g)  ⇌ 2NH3(g)

Question 6

Consider the following reaction and its equilibrium constant: I2(g)  + Br2(g)  ⇌ 2IBr(g)  Kc = 1.1 × 102
A reaction mixture contains 0.025 mol L-1 I2, 0.01 mol L-1 Br2, and 1.0 mol L-1 IBr. Which of the following statements is TRUE concerning this system?

Accepted Answer

A)   The reaction will shift in the direction of products.
B)   The reaction will shift in the direction of reactants.
C)   The reaction quotient will decrease.
D)   The equilibrium constant will increase.
E)   The system is at equilibrium.

Question 7

Dinitrogen tetroxide partially decomposes according to the following equilibrium: -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > (g)  ⇌ -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > (g)  A 1.000 L flask is charged with 6.00 × 10-2 mol of -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > . At equilibrium, 3.21 × 10-2 mol of -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > remains. -2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________. A)  10.3 mol L-1 B)  1.74 mol L-1 C)  0.465 mol L-1 D)  2.42 × 10-2 mol L-1 E)  9.70 × 10-2 mol L-1" class="answers-bank-image d-inline" rel="preload" > for this reaction is ________.

Accepted Answer

A)   10.3 mol L-1
B)   1.74 mol L-1
C)   0.465 mol L-1
D)   2.42 × 10-2 mol L-1
E)   9.70 × 10-2 mol L-1

Question 8

Match the following.
-K ≈ 1

Accepted Answer

A)  reverse reaction is favoured
B)  reaction is at equilibrium
C)  reaction favours formation of more products
D)  reaction does not strongly favour reactants or products
E)  reaction has a larger amount of products than reactantsF) reaction will favour formation of reactants

Question 9

The reaction below has a Kc value of 1.0 × 1012 M-1. What is the value of Kp for this reaction at 500 K? 2SO2(g)  + O2(g)  ⇌ 2SO3(g)

Accepted Answer

A)   4.2 × 10-11 bar-1
B)   1.0 × 1012 bar-1
C)   2.4 × 10-12 bar-1
D)   4.1 × 1013 bar-1
E)   2.4 × 1010 bar-1

Question 10

Consider the following reaction and its equilibrium constant: I2(g)  + Br2(g)  ⇌ 2IBr(g)  Kc = 1.1 × 102
A reaction mixture contains 0.5 mol L-1 I2, 1.0 mol L-1 Br2, and 2.0 mol L-1 IBr. Which of the following statements is TRUE concerning this system?

Accepted Answer

A)   The reaction will shift in the direction of products.
B)   The reaction will shift in the direction of reactants.
C)   The reaction quotient will decrease.
D)   The equilibrium constant will increase.
E)   The system is at equilibrium.

Question 11

Consider the following reaction: CH4(g)  + 2H2S(g)  ⇌ CS2(g)  + 4H2(g) 
A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1)  for the reaction.

Accepted Answer

A)   0.23 mol2 L-2
B)   0.038 mol2 L-2
C)   2.9 mol2 L-2
D)   10. mol2 L-2
E)   0.34 mol2 L-2

Question 12

Which of the following statements is TRUE about the implication of K >> 1?

Accepted Answer

A)   At equilibrium, the amount of products is favoured over the amount of reactants.
B)   At equilibrium, the amount of reactants is favoured over the amount of products.
C)   The rate of the reaction is favoured.
D)   The reverse reaction is favoured.
E)   Neither the forward nor reverse reaction is strongly favoured; the forward reaction proceeds about halfway.

Question 13

Consider the following reaction and its equilibrium constant: 4CuO(s)  + CH4(g)  ⇌ CO2(g)  + 4Cu(s)  + 2H2O(g)  Kc = 1.10
A reaction mixture contains 2.0 mol L-1 CH4, 0.25 mol L-1 CO2, and 0.5 mol L-1 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.

Question 14

Express the equilibrium constant for the following reaction: 2P(g)  + 3Cl2(g)  ⇌ 2PCl3(g)

Accepted Answer

A)   KP = 2(g)  ⇌ 2PCl3(g)  
A)   KP =   
B)   KP =   
C)   KP =   
D)   KP =   
E)   KP =  " class="answers-bank-image d-inline" rel="preload" >
B)   KP = 2(g)  ⇌ 2PCl3(g)  
A)   KP =   
B)   KP =   
C)   KP =   
D)   KP =   
E)   KP =  " class="answers-bank-image d-inline" rel="preload" >
C)   KP = 2(g)  ⇌ 2PCl3(g)  
A)   KP =   
B)   KP =   
C)   KP =   
D)   KP =   
E)   KP =  " class="answers-bank-image d-inline" rel="preload" >
D)   KP = 2(g)  ⇌ 2PCl3(g)  
A)   KP =   
B)   KP =   
C)   KP =   
D)   KP =   
E)   KP =  " class="answers-bank-image d-inline" rel="preload" >
E)   KP = 2(g)  ⇌ 2PCl3(g)  
A)   KP =   
B)   KP =   
C)   KP =   
D)   KP =   
E)   KP =  " class="answers-bank-image d-inline" rel="preload" >

Question 15

For the following reaction, what is △n required in the conversion of Kc to Kp? KClO3(s)  ⇌ KClO(s)  + O2(g)

Accepted Answer

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

Question 16

How is the reaction quotient different from an equilibrium constant for a given reaction?

Accepted Answer

The expressions for both are identical. ...

Question 17

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g) . N2O4(g)  ⇌ 2NO2(g)  Kc = 0.21 M
[N2O4]eq = 1.34 mol L-1

Accepted Answer

A)   0.25 mol L-1
B)   0.043 mol L-1
C)   0.60 mol L-1
D)   0.028 mol L-1
E)   0.53 mol L-1

Question 18

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm, P(NO) eq = 0.10 atm, P(Cl2) eq = 0.081 atm. 2NOCl(g)  ⇌ 2NO(g)  + Cl2(g)

Accepted Answer

A)   3.7 × 10-2 atm
B)   60 atm
C)   27 atm
D)   1.7 × 10-2 atm
E)   1.8 × 10-3 atm

Question 19

Express the equilibrium constant for the following reaction: B(OH) 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)

Accepted Answer

A)   Kc = 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)  
A)   Kc =   
B)   Kc =   
C)   Kc =   
D)   Kc =   
E)   Kc =  " class="answers-bank-image d-inline" rel="preload" >
B)   Kc = 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)  
A)   Kc =   
B)   Kc =   
C)   Kc =   
D)   Kc =   
E)   Kc =  " class="answers-bank-image d-inline" rel="preload" >
C)   Kc = 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)  
A)   Kc =   
B)   Kc =   
C)   Kc =   
D)   Kc =   
E)   Kc =  " class="answers-bank-image d-inline" rel="preload" >
D)   Kc = 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)  
A)   Kc =   
B)   Kc =   
C)   Kc =   
D)   Kc =   
E)   Kc =  " class="answers-bank-image d-inline" rel="preload" >
E)   Kc = 3(aq)  + 2H2O(l)  ⇌ B(OH) 3(OH) -(aq)  + H3O+(aq)  
A)   Kc =   
B)   Kc =   
C)   Kc =   
D)   Kc =   
E)   Kc =  " class="answers-bank-image d-inline" rel="preload" >

Question 20

Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9
If Kc = 0.143 at 25 °C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 mol L-1 and 0. 075 mol L-1, respectively.

Accepted Answer

A)   [C6H12] = 0. 041 mol L-1, [CH3C5H9] = 0. 041 mol L-1
B)   [C6H12] = 0. 159 mol L-1, [CH3C5H9] = 0. 116 mol L-1
C)   [C6H12] = 0. 241 mol L-1, [CH3C5H9] = 0. 034 mol L-1
D)   [C6H12] = 0. 253 mol L-1, [CH3C5H9] = 0. 022 mol L-1

Exam 14: Chemical Equilibrium

For the following reaction, what is △n required in the conversion of K_c to K_p? KClO₃(s) ⇌ KClO(s) + O₂(g)

Correct Answer
verified

K_c is 1.67 × 10²⁰ mol³ L^-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) If 0. 0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion, what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g) ⇌ (g) A 1.000 L flask is charged with 6.00 × 10^-2 mol of . At equilibrium, 3.21 × 10^-2 mol of remains. for this reaction is ________.

Correct Answer
verified

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.025 mol L^-1 I₂, 0.01 mol L^-1 Br₂, and 1.0 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

Correct Answer
verified

Correct Answer
verified

Express the equilibrium constant for the following reaction: SO₂₍_g₎ + H₂O(l) ⇌ H₂SO₃(aq)

Correct Answer
verified

The reaction below has a K_c value of 1.0 × 10¹²M^-1. What is the value of K_p for this reaction at 500 K? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Correct Answer
verified

For the following reaction, what is Δn required in the conversion of K_c to K_p? CH₄(g) + H₂O(g) ⇌ CO(g) + 3H₂(g)

Correct Answer
verified

How is the reaction quotient different from an equilibrium constant for a given reaction?

Correct Answer
verified
The expressions for both are identical. ...
View Answer

Express the equilibrium constant for the following reaction: 2P(g) + 3Cl₂(g) ⇌ 2PCl₃(g)

Correct Answer
verified

Which of the following statements is TRUE about the implication of K >> 1?

Correct Answer
verified

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm, P(NO) _eq = 0.10 atm, P(Cl₂) _eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl₂(g)

Correct Answer
verified

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH₄(g) ⇌ CO₂(g) + 4Cu(s) + 2H₂O(g) K_c = 1.10 A reaction mixture contains 2.0 mol L^-1 CH₄, 0.25 mol L^-1 CO₂, and 0.5 mol L^-1 H₂O. Which of the following statements is TRUE concerning this system?

Correct Answer
verified

Match the following. -K ≈ 1

Correct Answer
verified

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 1.34 mol L^-1

Correct Answer
verified

For which of the following reactions will K_c = K_p?

Correct Answer
verified

Consider the following reaction: 2H₂O(g) + 2SO₂(g) ⇌ 2H₂S(g) + 3O₂(g) A reaction mixture initially contains 2.8 mol L^-1 H₂O and 2.6 mol L^-1 SO₂. Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6mol L^-1.

Correct Answer
verified

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.5 mol L^-1 I₂, 1.0 mol L^-1 Br₂, and 2.0 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

Correct Answer
verified

Express the equilibrium constant for the following reaction: B(OH) ₃(aq) + 2H₂O(l) ⇌ B(OH) ₃(OH) ^-(aq) + H₃O⁺(aq)

Correct Answer
verified

Consider the following reaction: CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1) for the reaction.

Correct Answer
verified

Exam 14: Chemical Equilibrium

For the following reaction, what is △n required in the conversion of Kc to Kp? KClO3(s) ⇌ KClO(s) + O2(g)

Correct AnswerverifiedShow Answer

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) If 0. 0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

Correct AnswerverifiedShow Answer

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g) ⇌ (g) A 1.000 L flask is charged with 6.00 × 10-2 mol of . At equilibrium, 3.21 × 10-2 mol of remains. for this reaction is ________.

Correct AnswerverifiedShow Answer

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.025 mol L-1 I2, 0.01 mol L-1 Br2, and 1.0 mol L-1 IBr. Which of the following statements is TRUE concerning this system?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Express the equilibrium constant for the following reaction: SO2(g) + H2O(l) ⇌ H2SO3(aq)

Correct AnswerverifiedShow Answer

The reaction below has a Kc value of 1.0 × 1012 M-1. What is the value of Kp for this reaction at 500 K? 2SO2(g) + O2(g) ⇌ 2SO3(g)

Correct AnswerverifiedShow Answer

For the following reaction, what is Δn required in the conversion of Kc to Kp? CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g)

Correct AnswerverifiedShow Answer

How is the reaction quotient different from an equilibrium constant for a given reaction?

Correct AnswerverifiedThe expressions for both are identical. ...View AnswerShow Answer

Express the equilibrium constant for the following reaction: 2P(g) + 3Cl2(g) ⇌ 2PCl3(g)

Correct AnswerverifiedShow Answer

Which of the following statements is TRUE about the implication of K >> 1?

Correct AnswerverifiedShow Answer

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm, P(NO) eq = 0.10 atm, P(Cl2) eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

Correct AnswerverifiedShow Answer

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH4(g) ⇌ CO2(g) + 4Cu(s) + 2H2O(g) Kc = 1.10 A reaction mixture contains 2.0 mol L-1 CH4, 0.25 mol L-1 CO2, and 0.5 mol L-1 H2O. Which of the following statements is TRUE concerning this system?

Correct AnswerverifiedShow Answer

Match the following. -K ≈ 1

Correct AnswerverifiedShow Answer

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g) . N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M [N2O4]eq = 1.34 mol L-1

Correct AnswerverifiedShow Answer

For which of the following reactions will Kc = Kp?

Correct AnswerverifiedShow Answer

Consider the following reaction: 2H2O(g) + 2SO2(g) ⇌ 2H2S(g) + 3O2(g) A reaction mixture initially contains 2.8 mol L-1 H2O and 2.6 mol L-1 SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Correct AnswerverifiedShow Answer

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.5 mol L-1 I2, 1.0 mol L-1 Br2, and 2.0 mol L-1 IBr. Which of the following statements is TRUE concerning this system?

Correct AnswerverifiedShow Answer

Express the equilibrium constant for the following reaction: B(OH) 3(aq) + 2H2O(l) ⇌ B(OH) 3(OH) -(aq) + H3O+(aq)

Correct AnswerverifiedShow Answer

Consider the following reaction: CH4(g) + 2H2S(g) ⇌ CS2(g) + 4H2(g) A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1) for the reaction.

Correct AnswerverifiedShow Answer

For the following reaction, what is △n required in the conversion of K_c to K_p? KClO₃(s) ⇌ KClO(s) + O₂(g)

Correct Answer
verified

K_c is 1.67 × 10²⁰ mol³ L^-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) If 0. 0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion, what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g) ⇌ (g) A 1.000 L flask is charged with 6.00 × 10^-2 mol of . At equilibrium, 3.21 × 10^-2 mol of remains. for this reaction is ________.

Correct Answer
verified

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.025 mol L^-1 I₂, 0.01 mol L^-1 Br₂, and 1.0 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

Correct Answer
verified

Correct Answer
verified

Express the equilibrium constant for the following reaction: SO₂₍_g₎ + H₂O(l) ⇌ H₂SO₃(aq)

Correct Answer
verified

The reaction below has a K_c value of 1.0 × 10¹²M^-1. What is the value of K_p for this reaction at 500 K? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Correct Answer
verified

For the following reaction, what is Δn required in the conversion of K_c to K_p? CH₄(g) + H₂O(g) ⇌ CO(g) + 3H₂(g)

Correct Answer
verified

Correct Answer
verified
The expressions for both are identical. ...
View Answer

Express the equilibrium constant for the following reaction: 2P(g) + 3Cl₂(g) ⇌ 2PCl₃(g)

Correct Answer
verified

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Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm, P(NO) _eq = 0.10 atm, P(Cl₂) _eq = 0.081 atm. 2NOCl(g) ⇌ 2NO(g) + Cl₂(g)

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Consider the following reaction and its equilibrium constant: 4CuO(s) + CH₄(g) ⇌ CO₂(g) + 4Cu(s) + 2H₂O(g) K_c = 1.10 A reaction mixture contains 2.0 mol L^-1 CH₄, 0.25 mol L^-1 CO₂, and 0.5 mol L^-1 H₂O. Which of the following statements is TRUE concerning this system?

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Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 1.34 mol L^-1

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For which of the following reactions will K_c = K_p?

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Consider the following reaction: 2H₂O(g) + 2SO₂(g) ⇌ 2H₂S(g) + 3O₂(g) A reaction mixture initially contains 2.8 mol L^-1 H₂O and 2.6 mol L^-1 SO₂. Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6mol L^-1.

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Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.5 mol L^-1 I₂, 1.0 mol L^-1 Br₂, and 2.0 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

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Express the equilibrium constant for the following reaction: B(OH) ₃(aq) + 2H₂O(l) ⇌ B(OH) ₃(OH) ^-(aq) + H₃O⁺(aq)

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Consider the following reaction: CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1) for the reaction.

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