Question 1

At a certain temperature the reaction CO2(g)  + H2(g)  2(g)  + H2(g)    CO(g)  + H2O(g) 2 Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide? A)  0.091 M B)  0.191 M C)  0.209 M D)  0.913 M E)  1.05 M" class="answers-bank-image d-inline" rel="preload" > CO(g)  + H2O(g) 2
Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Accepted Answer

A)   0.091 M
B)   0.191 M
C)   0.209 M
D)   0.913 M
E)   1.05 M

Question 2

Unless ΔH°rxn = 0, a change in temperature will affect the value of the equilibrium constant Kc.

Accepted Answer

A) True 
 B)False

Question 3

Write the mass-action expression, 2(g)    NOBr(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > c, for the following chemical reaction. NO(g)  + ½Br2(g)  2(g)    NOBr(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > NOBr(g)

Accepted Answer

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

Question 4

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g)  2(g)    2NO(g)  + O2(g)  ΔH°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen? A)  high temperature, high pressure B)  low temperature, high pressure C)  high temperature, low pressure D)  low temperature, low pressure E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + O2(g)  ΔH°rxn = +114 kJ
Under which reaction conditions would you expect to produce the largest amount of oxygen?

Accepted Answer

A)   high temperature, high pressure
B)   low temperature, high pressure
C)   high temperature, low pressure
D)   low temperature, low pressure
E)   None of these choices are correct.

Question 5

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g)  + O2(g)  2(g)  + O2(g)    2NO(g)  The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen? A)  0.16 atm B)  0.31 atm C)  3.1 atm D)  7.7 atm E)  7.8 atm" class="answers-bank-image d-inline" rel="preload" > 2NO(g) 
The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

Accepted Answer

A)   0.16 atm
B)   0.31 atm
C)   3.1 atm
D)   7.7 atm
E)   7.8 atm

Question 6

Consider the reversible reaction: 2NO2(g)  2(g)    N2O4(g)  If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of        c? 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 0.016 mol L-1, what is the value of  2(g)    N2O4(g)  If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of        c? A)  0.016 B)  0.50 C)  1.0 D)  2.0 E)  63" class="answers-bank-image d-inline" rel="preload" >  
 
c?

Accepted Answer

A)   0.016
B)   0.50
C)   1.0
D)   2.0
E)   63

Question 7

Write the mass-action expression, +(aq)    Zn2+(aq)  + 2Ag(s)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  +(aq)    Zn2+(aq)  + 2Ag(s)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > Zn2+(aq)  + 2Ag(s)

Accepted Answer

A)   +(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   +(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   +(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   +(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   +(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 8

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s)  + CO2(g)  2(g)    NaHCO3(s)  Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium? A)  adding N2 gas to double the pressure B)  adding more solid NaOH C)  decreasing the volume of the container D)  removing half of the solid NaHCO3 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > NaHCO3(s) 
Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

Accepted Answer

A)   adding N2 gas to double the pressure
B)   adding more solid NaOH
C)   decreasing the volume of the container
D)   removing half of the solid NaHCO3
E)   None of these choices are correct.

Question 9

A chemical reaction will reach equilibrium when the limiting reactant is used up.

Accepted Answer

A) True 
 B)False

Question 10

At high temperatures, carbon reacts with O2 to produce CO as follows: C(s)  + O2(g)  2 to produce CO as follows: C(s)  + O2(g)    2CO(g) . When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction? A)  0.010 B)  0.072 C)  0.090 D)  0.17 E)  1.2" class="answers-bank-image d-inline" rel="preload" > 2CO(g) .
When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?

Accepted Answer

A)   0.010
B)   0.072
C)   0.090
D)   0.17
E)   1.2

Question 11

The reaction quotient, c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate? A)  The reaction must proceed to the left to establish equilibrium. B)  The reaction must proceed to the right to establish equilibrium. C)  The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium. D)  The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium. E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?

Accepted Answer

A)   The reaction must proceed to the left to establish equilibrium.
B)   The reaction must proceed to the right to establish equilibrium.
C)   The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D)   The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E)   None of these choices are correct.

Question 12

Consider the equilibrium reaction: N2O4(g)  2O4(g)    2NO2(g)  Which of the following correctly describes the relationship between Kc and Kp for the reaction? A)  Kp = Kc B)  Kp = RT × Kc C)  Kp = (RT × Kc) -1 D)  Kp = Kc / RT E)  Kp = RT / Kc" class="answers-bank-image d-inline" rel="preload" > 2NO2(g)  Which of the following correctly describes the relationship between Kc and Kp for the reaction?

Accepted Answer

A)   Kp = Kc
B)   Kp = RT × Kc
C)   Kp = (RT × Kc) -1
D)   Kp = Kc / RT
E)   Kp = RT / Kc

Question 13

In water, the following equilibrium exists: H+(aq)  + OH-(aq)  +(aq)  + OH-(aq)    H2O(l)  In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above. A)  1.00 × 1014 B)  1.00 × 1012 C)  1.00 × 10-14 D)  1.00 × 10-12 E)  5.55 × 1015" class="answers-bank-image d-inline" rel="preload" > H2O(l) 
In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Accepted Answer

A)   1.00 × 1014
B)   1.00 × 1012
C)   1.00 × 10-14
D)   1.00 × 10-12
E)   5.55 × 1015

Question 14

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g)  3) 3COH(g)    (CH3) 2CCH2(g)  + H2O(g)  A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature? A)  The forward reaction will proceed to reestablish equilibrium. B)  The reverse reaction will proceed to reestablish equilibrium. C)  No change occurs. D)  The equilibrium constant will increase. E)  The equilibrium constant will decrease." class="answers-bank-image d-inline" rel="preload" > (CH3) 2CCH2(g)  + H2O(g) 
A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Accepted Answer

A)   The forward reaction will proceed to reestablish equilibrium.
B)   The reverse reaction will proceed to reestablish equilibrium.
C)   No change occurs.
D)   The equilibrium constant will increase.
E)   The equilibrium constant will decrease.

Question 15

At 850°C, the equilibrium constant Kp for the reaction C(s)  + CO2(g)  2(g)    2CO(g)  Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide? A)  0.362 atm B)  0.489 atm C)  0.667 atm D)  0.915 atm E)  0.921 atm" class="answers-bank-image d-inline" rel="preload" > 2CO(g) 
Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Accepted Answer

A)   0.362 atm
B)   0.489 atm
C)   0.667 atm
D)   0.915 atm
E)   0.921 atm

Question 16

Compounds A, B, and C react according to the following equation. 3A(g)  + 2B(g)  c for this reaction? A)  0.309 B)  0.601 C)  1.66 D)  3.24 E)  > 10" class="answers-bank-image d-inline" rel="preload" > 2C(g) 
At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?

Accepted Answer

A)   0.309
B)   0.601
C)   1.66
D)   3.24
E)   > 10

Question 17

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g)  + 2H2(g)  2(g)    CH3OH(g)  ΔH°rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C? A)  All the partial pressures will decrease. B)  The partial pressure of methanol will decrease. C)  The partial pressures of hydrogen and methanol will decrease. D)  The partial pressure of hydrogen will increase. E)  The partial pressure of carbon monoxide will decrease." class="answers-bank-image d-inline" rel="preload" > CH3OH(g)  ΔH°rxn = -90.7 kJ
A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

Accepted Answer

A)   All the partial pressures will decrease.
B)   The partial pressure of methanol will decrease.
C)   The partial pressures of hydrogen and methanol will decrease.
D)   The partial pressure of hydrogen will increase.
E)   The partial pressure of carbon monoxide will decrease.

Question 18

The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when

Accepted Answer

A)   all of the reactants and products are gases.
B)   in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.
C)   in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.
D)   in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.
E)   in the reaction equation, the total number of moles of reactants equals that of the products.

Question 19

For some gas-phase reactions, Kp = Kc.

Accepted Answer

A) True 
 B)False

Question 20

At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g)  p, is 4.00 × 10-4 for the equilibrium: 2HCN(g)    H2(g)  + C2N2(g)  What is Kp for the following reaction? H2(g)  + C2N2(g)    2HCN(g)  A)  2.00 × 10-4 B)  -4.00 × 10-4 C)  1.25 × 103 D)  2.50 × 103 E)  4.00 × 104" class="answers-bank-image d-inline" rel="preload" > H2(g)  + C2N2(g) 
What is Kp for the following reaction?
H2(g)  + C2N2(g)  p, is 4.00 × 10-4 for the equilibrium: 2HCN(g)    H2(g)  + C2N2(g)  What is Kp for the following reaction? H2(g)  + C2N2(g)    2HCN(g)  A)  2.00 × 10-4 B)  -4.00 × 10-4 C)  1.25 × 103 D)  2.50 × 103 E)  4.00 × 104" class="answers-bank-image d-inline" rel="preload" > 2HCN(g)

Accepted Answer

A)   2.00 × 10-4
B)   -4.00 × 10-4
C)   1.25 × 103
D)   2.50 × 103
E)   4.00 × 104

Exam 17: Equilibrium the Extent of Chemical Reactions

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Correct Answer
verified

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Correct Answer
verified

Correct Answer
verified

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

Correct Answer
verified

The reaction quotient, _c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

Correct Answer
verified

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br₂(g) NOBr(g)

Correct Answer
verified

Unless ΔH°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

Correct Answer
verified

A chemical reaction will reach equilibrium when the limiting reactant is used up.

Correct Answer
verified

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

Correct Answer
verified

For some gas-phase reactions, K_p = K_c.

Correct Answer
verified

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

Correct Answer
verified

Correct Answer
verified

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

Correct Answer
verified

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) ₂ Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Correct Answer
verified

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃) ₃COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct Answer
verified

At 500°C the equilibrium constant, K_p, is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is Kp for the following reaction? H₂(g) + C₂N₂(g) 2HCN(g)

Correct Answer
verified

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are 0.016 mol L^-1, what is the value of _c?

Correct Answer
verified

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) ΔH°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

Correct Answer
verified

The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

Correct Answer
verified

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H₂(g) CH₃OH(g) ΔH°_rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

Correct Answer
verified

Exam 17: Equilibrium the Extent of Chemical Reactions

In water, the following equilibrium exists: H+(aq) + OH-(aq) H2O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Correct AnswerverifiedShow Answer

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO2(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Correct AnswerverifiedShow Answer

At high temperatures, carbon reacts with O2 to produce CO as follows: C(s) + O2(g) 2CO(g) . When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?

Correct AnswerverifiedShow Answer

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?

Correct AnswerverifiedShow Answer

The reaction quotient, c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?

Correct AnswerverifiedShow Answer

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br2(g) NOBr(g)

Correct AnswerverifiedShow Answer

Unless ΔH°rxn = 0, a change in temperature will affect the value of the equilibrium constant Kc.

Correct AnswerverifiedShow Answer

A chemical reaction will reach equilibrium when the limiting reactant is used up.

Correct AnswerverifiedShow Answer

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

Correct AnswerverifiedShow Answer

For some gas-phase reactions, Kp = Kc.

Correct AnswerverifiedShow Answer

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?

Correct AnswerverifiedShow Answer

At a certain temperature the reaction CO2(g) + H2(g) CO(g) + H2O(g) 2 Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Correct AnswerverifiedShow Answer

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g) (CH3) 2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct AnswerverifiedShow Answer

At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) 2HCN(g)

Correct AnswerverifiedShow Answer

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of c?

Correct AnswerverifiedShow Answer

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) ΔH°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

Correct AnswerverifiedShow Answer

The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when

Correct AnswerverifiedShow Answer

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) CH3OH(g) ΔH°rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

Correct AnswerverifiedShow Answer

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Correct Answer
verified

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Correct Answer
verified

Correct Answer
verified

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

Correct Answer
verified

The reaction quotient, _c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

Correct Answer
verified

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br₂(g) NOBr(g)

Correct Answer
verified

Unless ΔH°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

Correct Answer
verified

Correct Answer
verified

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

Correct Answer
verified

For some gas-phase reactions, K_p = K_c.

Correct Answer
verified

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

Correct Answer
verified

Correct Answer
verified

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

Correct Answer
verified

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) ₂ Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Correct Answer
verified

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃) ₃COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct Answer
verified

At 500°C the equilibrium constant, K_p, is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is Kp for the following reaction? H₂(g) + C₂N₂(g) 2HCN(g)

Correct Answer
verified

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are 0.016 mol L^-1, what is the value of _c?

Correct Answer
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Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) ΔH°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

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The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

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Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H₂(g) CH₃OH(g) ΔH°_rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

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