Question 1

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g)  + Cl2(g)  2(g)  + Cl2(g)    2BrCl(g)  What is the equilibrium constant for the following reaction? BrCl(g)      Br2(g)  +   Cl2(g)  A)  2.97 × 10-4 B)  1.72 × 10-2 C)  3.45 × 10-2 D)  1.31 × 10-1 E)  > 1.00" class="answers-bank-image d-inline" rel="preload" > 2BrCl(g) 
What is the equilibrium constant for the following reaction?
BrCl(g)  2(g)  + Cl2(g)    2BrCl(g)  What is the equilibrium constant for the following reaction? BrCl(g)      Br2(g)  +   Cl2(g)  A)  2.97 × 10-4 B)  1.72 × 10-2 C)  3.45 × 10-2 D)  1.31 × 10-1 E)  > 1.00" class="answers-bank-image d-inline" rel="preload" > 2(g)  + Cl2(g)    2BrCl(g)  What is the equilibrium constant for the following reaction? BrCl(g)      Br2(g)  +   Cl2(g)  A)  2.97 × 10-4 B)  1.72 × 10-2 C)  3.45 × 10-2 D)  1.31 × 10-1 E)  > 1.00" class="answers-bank-image d-inline" rel="preload" > Br2(g)  + 2(g)  + Cl2(g)    2BrCl(g)  What is the equilibrium constant for the following reaction? BrCl(g)      Br2(g)  +   Cl2(g)  A)  2.97 × 10-4 B)  1.72 × 10-2 C)  3.45 × 10-2 D)  1.31 × 10-1 E)  > 1.00" class="answers-bank-image d-inline" rel="preload" > Cl2(g)

Accepted Answer

A)   2.97 × 10-4
B)   1.72 × 10-2
C)   3.45 × 10-2
D)   1.31 × 10-1
E)   > 1.00F) D) and E)
G) A) and B)

Question 2

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)   > 10F) B) and C)
G) None of the above

Question 3

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change Kp.

Accepted Answer

A) True 
 B)False

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? A)  1.81 × 10-16 B)  1.83 × 10-14 C)  4.48 × 10-13 D)  1.10 × 10-11 E)  1.11 × 10-9" 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?

Accepted Answer

A)   1.81 × 10-16
B)   1.83 × 10-14
C)   4.48 × 10-13
D)   1.10 × 10-11
E)   1.11 × 10-9F) A) and C)
G) C) and D)

Question 5

Consider the equilibrium reaction shown below. B2(g)  2(g)      2B(g)  If the rate constants are: kfwd = 7.00 × 10-5 s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions? A)  1.75 × 105 B)  3.50 C)  0.286 D)  5.71 × 10-6 E)  1.40 × 10-10" class="answers-bank-image d-inline" rel="preload" >  
2B(g) 
If the rate constants are: kfwd = 7.00 × 10-5 s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?

Accepted Answer

A)   1.75 × 105
B)   3.50
C)   0.286
D)   5.71 × 10-6
E)   1.40 × 10-10F) C) and D)
G) A) and D)

Question 6

A mixture 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 the value of Kc for this reaction? CO(g)  + Br2(g)  2 was 0.233 M. What is the value of Kc for this reaction? CO(g)  + Br2(g)    COBr2(g)  A)  5.23 B)  1.22 C)  1.165 D)  0.858 E)  0.191" class="answers-bank-image d-inline" rel="preload" > COBr2(g)

Accepted Answer

A)   5.23
B)   1.22
C)   1.165
D)   0.858
E)   0.191F) D) and E)
G) A) and D)

Question 7

Hydrogen sulfide can be formed in the following reaction: H2(g)  + 2(g)  +   S2(g)    H2S(g)  H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K. A)  5.05 B)  18.8 C)  34.7 D)  88.9 E)  598" class="answers-bank-image d-inline" rel="preload" > S2(g)  2(g)  +   S2(g)    H2S(g)  H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K. A)  5.05 B)  18.8 C)  34.7 D)  88.9 E)  598" class="answers-bank-image d-inline" rel="preload" > H2S(g)  H°rxn = -92 kJ
The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.

Accepted Answer

A)   5.05
B)   18.8
C)   34.7
D)   88.9
E)   598F) A) and C)
G) D) and E)

Question 8

Hydrogen sulfide will react with water as shown in the following reactions. H2S(g)  + H2O(l)  2S(g)  + H2O(l)    H3O+(aq)  + HS-(aq)  K1 = 1.0 × 10-7 HS-(aq)  + H2O(l)    H3O+(aq)  + S2-(aq)  K2 = ? H2S(g)  + 2H2O(l)    2H3O+(aq)  + S2-(aq)  K3 = 1.3 × 10-20 What is the value of K2? A)  1.3 × 10-27 B)  2.3 × 10-7 C)  1.3 × 10-13 D)  7.7 × 1012 E)  7.7 × 1026" class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + HS-(aq)  K1 = 1.0 × 10-7
HS-(aq)  + H2O(l)  2S(g)  + H2O(l)    H3O+(aq)  + HS-(aq)  K1 = 1.0 × 10-7 HS-(aq)  + H2O(l)    H3O+(aq)  + S2-(aq)  K2 = ? H2S(g)  + 2H2O(l)    2H3O+(aq)  + S2-(aq)  K3 = 1.3 × 10-20 What is the value of K2? A)  1.3 × 10-27 B)  2.3 × 10-7 C)  1.3 × 10-13 D)  7.7 × 1012 E)  7.7 × 1026" class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + S2-(aq)  K2 = ?
H2S(g)  + 2H2O(l)  2S(g)  + H2O(l)    H3O+(aq)  + HS-(aq)  K1 = 1.0 × 10-7 HS-(aq)  + H2O(l)    H3O+(aq)  + S2-(aq)  K2 = ? H2S(g)  + 2H2O(l)    2H3O+(aq)  + S2-(aq)  K3 = 1.3 × 10-20 What is the value of K2? A)  1.3 × 10-27 B)  2.3 × 10-7 C)  1.3 × 10-13 D)  7.7 × 1012 E)  7.7 × 1026" class="answers-bank-image d-inline" rel="preload" > 2H3O+(aq)  + S2-(aq)  K3 = 1.3 × 10-20
What is the value of K2?

Accepted Answer

A)   1.3 × 10-27
B)   2.3 × 10-7
C)   1.3 × 10-13
D)   7.7 × 1012
E)   7.7 × 1026F) B) and D)
G) B) and E)

Question 9

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 the above" 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 the aboveF) All of the above
G) B) and D)

Question 10

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 1.5 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) 
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 MF) A) and D)
G) A) and B)

Question 11

The equilibrium constant, Kp , for the reaction CO(g)  + H2O(g)  p , for the reaction CO(g)  + H2O(g)    CO2(g)  + H2(g)  At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium? A)  Yes. B)  No, the forward reaction must proceed to establish equilibrium. C)  No, the reverse reaction must proceed to establish equilibrium. D)  Need to know the volume of the container before deciding. E)  Need to know the starting concentrations of all substances before deciding." class="answers-bank-image d-inline" rel="preload" > CO2(g)  + H2(g) 
At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Accepted Answer

A)   Yes.
B)   No, the forward reaction must proceed to establish equilibrium.
C)   No, the reverse reaction must proceed to establish equilibrium.
D)   Need to know the volume of the container before deciding.
E)   Need to know the starting concentrations of all substances before deciding.F) All of the above
G) A) and B)

Question 12

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

Accepted Answer

A) True 
 B)False

Question 13

The reaction quotient, Qc, 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 the above statements is accurate.F) C) and D)
G) All of the above

Question 14

Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH) 2(s)  2(s)    Mg2+(aq)  + 2OH-(aq)  The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH) 2 are now added to the mixture? A)  The hydroxide ion concentration will decrease. B)  The hydroxide ion concentration will increase. C)  The hydroxide ion concentration will be unchanged. D)  The solution will become supersaturated. E)  None of the above conclusions is justified without additional information." class="answers-bank-image d-inline" rel="preload" > Mg2+(aq)  + 2OH-(aq) 
The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH) 2 are now added to the mixture?

Accepted Answer

A)   The hydroxide ion concentration will decrease.
B)   The hydroxide ion concentration will increase.
C)   The hydroxide ion concentration will be unchanged.
D)   The solution will become supersaturated.
E)   None of the above conclusions is justified without additional information.F) A) and B)
G) A) and C)

Question 15

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/KcF) C) and D)
G) B) and C)

Question 16

The equilibrium constant Kc for the reaction A(g)  + B(g)  c for the reaction A(g)  + B(g)    C(g)  Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C? A)  0.19 M B)  0.29 M C)  0.36 M D)  0.41 M E)  0.51 M" class="answers-bank-image d-inline" rel="preload" > C(g) 
Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

Accepted Answer

A)   0.19 M
B)   0.29 M
C)   0.36 M
D)   0.41 M
E)   0.51 MF) A) and D)
G) None of the above

Question 17

Consider the following gas-phase equilibrium reaction:
N2(g) + O2(g)  2NO(g) Kc = 4.10 × 10-4 at 2000°C
If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

Accepted Answer

[NO] = 1.0...

Question 18

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

Accepted Answer

A)   c, for the following chemical reaction. NO(g)  +   Br2(g)    NOBr(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c, for the following chemical reaction. NO(g)  +   Br2(g)    NOBr(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c, for the following chemical reaction. NO(g)  +   Br2(g)    NOBr(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c, for the following chemical reaction. NO(g)  +   Br2(g)    NOBr(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c, for the following chemical reaction. NO(g)  +   Br2(g)    NOBr(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) C) and D)

Question 19

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g)  2(g)    2NO(g)  + O2(g)  H°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 the above, unless a catalyst is present" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + O2(g)  H°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 the above, unless a catalyst is presentF) C) and E)
G) B) and D)

Question 20

A chemical reaction has an equilibrium constant of 2 × 106. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

Accepted Answer

A)   The forward and back reactions have stopped.
B)   The limiting reactant has been used up.
C)   The forward and reverse rate constants are equal.
D)   The forward and reverse reaction rates are equal.
E)   None of the above conclusions is correct.F) A) and D)
G) A) and C)

Exam 17: Equilibrium: the Extent of Chemical Reactions

Consider the following gas-phase equilibrium reaction: N₂(g) + O₂(g) 2NO(g) K_c = 4.10 × 10^-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

Correct Answer
verified
[NO] = 1.0...
View Answer

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

Correct Answer
verified

A mixture 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 COBr₂was 0.233 M. What is the value of K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

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?

Correct Answer
verified

Consider the equilibrium reaction shown below. B₂(g) 2B(g) If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Correct Answer
verified

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Correct Answer
verified

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^-(aq) K₁= 1.0 × 10^-7 HS^-(aq) + H₂O(l) H₃O⁺(aq) + S^2-(aq) K₂= ? H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2-(aq) K₃= 1.3 × 10^-20 What is the value of K₂?

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

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

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change K_p.

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

Correct Answer
verified

The equilibrium constant K_c for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

Correct Answer
verified

A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

Correct Answer
verified

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

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 1.5 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

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) H°_rxn = -92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Correct Answer
verified

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

Correct Answer
verified

The reaction quotient, Q_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

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br₂(g) + Cl₂(g)

Correct Answer
verified

Exam 17: Equilibrium: the Extent of Chemical Reactions

Consider the following gas-phase equilibrium reaction: N2(g) + O2(g) 2NO(g) Kc = 4.10 × 10-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

Correct Answerverified[NO] = 1.0...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

A mixture 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 the value of Kc for this reaction? CO(g) + Br2(g) COBr2(g)

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?

Correct AnswerverifiedShow Answer

Consider the equilibrium reaction shown below. B2(g) 2B(g) If the rate constants are: kfwd = 7.00 × 10-5 s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?

Correct AnswerverifiedShow Answer

The equilibrium constant, Kp , for the reaction CO(g) + H2O(g) CO2(g) + H2(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Correct AnswerverifiedShow Answer

Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7 HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) K2 = ? H2S(g) + 2H2O(l) 2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20 What is the value of K2?

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

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

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change Kp.

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

Correct AnswerverifiedShow Answer

The equilibrium constant Kc for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

Correct AnswerverifiedShow Answer

A chemical reaction has an equilibrium constant of 2 × 106. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

Correct AnswerverifiedShow Answer

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

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 1.5 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

Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.

Correct AnswerverifiedShow Answer

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

Correct AnswerverifiedShow Answer

The reaction quotient, Qc, 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

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br2(g) + Cl2(g)

Correct AnswerverifiedShow Answer

Consider the following gas-phase equilibrium reaction: N₂(g) + O₂(g) 2NO(g) K_c = 4.10 × 10^-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

Correct Answer
verified
[NO] = 1.0...
View Answer

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

Correct Answer
verified

A mixture 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 COBr₂was 0.233 M. What is the value of K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

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?

Correct Answer
verified

Consider the equilibrium reaction shown below. B₂(g) 2B(g) If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Correct Answer
verified

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Correct Answer
verified

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^-(aq) K₁= 1.0 × 10^-7 HS^-(aq) + H₂O(l) H₃O⁺(aq) + S^2-(aq) K₂= ? H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2-(aq) K₃= 1.3 × 10^-20 What is the value of K₂?

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

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

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change K_p.

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

Correct Answer
verified

The equilibrium constant K_c for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

Correct Answer
verified

A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

Correct Answer
verified

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

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 1.5 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

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) H°_rxn = -92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Correct Answer
verified

Correct Answer
verified

The reaction quotient, Q_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

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br₂(g) + Cl₂(g)

Correct Answer
verified