Question 1

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, NO = 0.526 atm,   = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g)  + Br2(g)    2NOBr(g)  A)  7.45 × 10-3 B)  0.109 C)  9.18 D)  91.8 E)  134" class="answers-bank-image d-inline" rel="preload" > = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction.
2NO(g)  + Br2(g)  NO = 0.526 atm,   = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g)  + Br2(g)    2NOBr(g)  A)  7.45 × 10-3 B)  0.109 C)  9.18 D)  91.8 E)  134" class="answers-bank-image d-inline" rel="preload" > 2NOBr(g)

Accepted Answer

A)   7.45 × 10-3
B)   0.109
C)   9.18
D)   91.8
E)   134F) None of the above
G) B) and E)

Question 2

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, Kc.

Accepted Answer

A) True 
 B)False

Question 3

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)    ½Br2(g)  + ½Cl2(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)    ½Br2(g)  + ½Cl2(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" > ½Br2(g)  + ½Cl2(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) A) and D)
G) C) and E)

Question 4

H2SO3(aq)  2SO3(aq)    HSO3(aq)  + H+(aq)  Kc = 1.4 × 10-2 H2SO3(aq)    SO32-(aq)  + 2H+(aq)  Kc = 9.1 × 10-10 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction HSO3-(aq)    SO32-(aq)  + H+(aq) ? A)  6.5 ×10-8 B)  1.3 × 10-11 C)  7.8 × 1010 D)  1.5 × 107 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > HSO3(aq)  + H+(aq)  Kc = 1.4 × 10-2 H2SO3(aq)  2SO3(aq)    HSO3(aq)  + H+(aq)  Kc = 1.4 × 10-2 H2SO3(aq)    SO32-(aq)  + 2H+(aq)  Kc = 9.1 × 10-10 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction HSO3-(aq)    SO32-(aq)  + H+(aq) ? A)  6.5 ×10-8 B)  1.3 × 10-11 C)  7.8 × 1010 D)  1.5 × 107 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > SO32-(aq)  + 2H+(aq)  Kc = 9.1 × 10-10
Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
HSO3-(aq)  2SO3(aq)    HSO3(aq)  + H+(aq)  Kc = 1.4 × 10-2 H2SO3(aq)    SO32-(aq)  + 2H+(aq)  Kc = 9.1 × 10-10 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction HSO3-(aq)    SO32-(aq)  + H+(aq) ? A)  6.5 ×10-8 B)  1.3 × 10-11 C)  7.8 × 1010 D)  1.5 × 107 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > SO32-(aq)  + H+(aq) ?

Accepted Answer

A)   6.5 ×10-8
B)   1.3 × 10-11
C)   7.8 × 1010
D)   1.5 × 107
E)   None of these choices are correct.F) D) and E)
G) B) and C)

Question 5

10.0 mL of a 0.100 mol L-1 solution of a metal ion M2+ is mixed with 10.0 mL of a 0.100 mol L-1 solution of a substance L. The following equilibrium is established: M2+(aq)  + 2L(aq)  -1 solution of a metal ion M2+ is mixed with 10.0 mL of a 0.100 mol L-1 solution of a substance L. The following equilibrium is established: M2+(aq)  + 2L(aq)    ML22+(aq)  At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1? A)  0.100 mol L-1 B)  0.050 mol L-1 C)  0.025 mol L-1 D)  0.0200 mol L-1 E)  0.0100 mol L-1" class="answers-bank-image d-inline" rel="preload" > ML22+(aq) 
At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1?

Accepted Answer

A)   0.100 mol L-1
B)   0.050 mol L-1
C)   0.025 mol L-1
D)   0.0200 mol L-1
E)   0.0100 mol L-1F) All of the above
G) B) and D)

Question 6

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 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) A) and B)
G) A) and D)

Question 7

Chemical reactions generally reach equilibrium because one of the reactants is used up.

Accepted Answer

A) True 
 B)False

Question 8

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 these choices are correct." 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 these choices are correct.F) C) and D)
G) B) and C)

Question 9

The equilibrium constant for reaction (1)  below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1)  ½X2(g)  + ½Y2(g)  2(g)  + ½Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > XY(g) 
(2)  2XY(g)  2(g)  + ½Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > X2(g)  + Y2(g)

Accepted Answer

A)   6.02 × 10-2
B)   7.25 × 10-3
C)   3.62 × 10-3
D)   1.31 × 10-5
E)   None of these choices are correct.F) A) and B)
G) B) and E)

Question 10

What is the mass-action expression, 2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  A)    B)    C)    D)    E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > c, for the following chemical reaction? Cu2+(aq)  + 4NH3(aq)  2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  A)    B)    C)    D)    E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > Cu(NH3) 42+(aq)

Accepted Answer

A)   2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
B)   2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
C)   2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
D)   2+(aq)  + 4NH3(aq)    Cu(NH3) 42+(aq)  
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
E)   None of these choices are correct.F) A) and E)
G) A) and D)

Question 11

Sodium hydrogen carbonate decomposes above 110°C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s)  3(s)    Na2CO3(s)  + H2O(g)  + CO2(g)  One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added? A)  The partial pressure of carbon dioxide will increase. B)  The partial pressure of carbon dioxide will decrease. C)  The partial pressure of carbon dioxide will be unchanged. D)  The amounts of all products will be greater when equilibrium is reestablished. E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > Na2CO3(s)  + H2O(g)  + CO2(g) 
One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?

Accepted Answer

A)   The partial pressure of carbon dioxide will increase.
B)   The partial pressure of carbon dioxide will decrease.
C)   The partial pressure of carbon dioxide will be unchanged.
D)   The amounts of all products will be greater when equilibrium is reestablished.
E)   None of these choices are correct.F) All of the above
G) C) and D)

Question 12

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g)  + 2H2(g)  2(g)    CH3OH(g)  A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm? A)  The partial pressure of hydrogen will decrease. B)  The partial pressure of hydrogen will increase. C)  The partial pressure of hydrogen will be unchanged. D)  Kp needs to be known before a prediction can be made. E)  Both Kp and the temperature need to be known before a prediction can be made." class="answers-bank-image d-inline" rel="preload" > CH3OH(g) 
A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?

Accepted Answer

A)   The partial pressure of hydrogen will decrease.
B)   The partial pressure of hydrogen will increase.
C)   The partial pressure of hydrogen will be unchanged.
D)   Kp needs to be known before a prediction can be made.
E)   Both Kp and the temperature need to be known before a prediction can be made.F) A) and B)
G) All of the above

Question 13

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s)  4I(s)    NH3(g)  + HI(g)  At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C. A)  0.103 atm B)  0.215 atm C)  0.232 atm D)  0.464 atm E)  2.00 atm" class="answers-bank-image d-inline" rel="preload" > NH3(g)  + HI(g) 
At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Accepted Answer

A)   0.103 atm
B)   0.215 atm
C)   0.232 atm
D)   0.464 atm
E)   2.00 atmF) A) and B)
G) B) and E)

Question 14

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, Kc, will also be doubled.

Accepted Answer

A) True 
 B)False

Question 15

Write the mass-action expression,          c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" >    
c, for the following chemical reaction equation.
2C6H6(g)  + 15O2(g)          c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 12CO2(g)  + 6H2O(g)

Accepted Answer

A)           c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)           c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)           c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)           c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)           c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) None of the above
G) All of the above

Question 16

The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s)  4.5H2O(s)    CuSO4(s)  + 5H2O(g)  Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium? A)  increasing the volume of the container B)  decreasing the volume of the container C)  adding a catalyst D)  removing some solid CuSO4 E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > CuSO4(s)  + 5H2O(g) 
Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?

Accepted Answer

A)   increasing the volume of the container
B)   decreasing the volume of the container
C)   adding a catalyst
D)   removing some solid CuSO4
E)   None of these choices are correct.F) A) and B)
G) A) and C)

Question 17

Which of the following has an effect on the magnitude of the equilibrium constant?

Accepted Answer

A)   removing products as they are formed
B)   adding more of a reactant
C)   adding a catalyst
D)   increasing the pressure, in a gas-phase reaction
E)   change in temperatureF) A) and B)
G) A) and D)

Question 18

In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant Kc will also increase.

Accepted Answer

A) True 
 B)False

Question 19

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 these choices are correct.F) A) and D)
G) A) and C)

Question 20

Consider the following two equilibria and their respective equilibrium constants: (1)  NO(g)  + ½O2(g)  2(g)    2NO(g)  + O2(g)  Which one of the following is the correct relationship between the equilibrium constants K1 and K2? A)  K2 = 2/K1 B)  K2 = (1/K1) 2 C)  K2 = -K1/2 D)  K2 = 1/(2K1)  E)  K2 = 1/(2K1) 2" class="answers-bank-image d-inline" rel="preload" > NO2(g) 
(2)  2NO2(g)  2(g)    2NO(g)  + O2(g)  Which one of the following is the correct relationship between the equilibrium constants K1 and K2? A)  K2 = 2/K1 B)  K2 = (1/K1) 2 C)  K2 = -K1/2 D)  K2 = 1/(2K1)  E)  K2 = 1/(2K1) 2" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + O2(g) 
Which one of the following is the correct relationship between the equilibrium constants K1 and K2?

Accepted Answer

A)   K2 = 2/K1
B)   K2 = (1/K1) 2
C)   K2 = -K1/2
D)   K2 = 1/(2K1) 
E)   K2 = 1/(2K1) 2F) B) and D)
G) A) and C)

Exam 17: Equilibrium the Extent of Chemical Reactions

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) ½Br₂(g) + ½Cl₂(g)

Correct Answer
verified

H₂SO₃(aq) HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10^-2 H₂SO₃(aq) SO₃^2-(aq) + 2H⁺(aq) K_c = 9.1 × 10^-10 Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction HSO₃^-(aq) SO₃^2-(aq) + H⁺(aq) ?

Correct Answer
verified

Correct Answer
verified

Which of the following has an effect on the magnitude of the equilibrium constant?

Correct Answer
verified

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) NO2(g) (2) 2NO₂(g) 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

Correct Answer
verified

What is the mass-action expression, c, for the following chemical reaction? Cu₂₊(aq) + 4NH₃(aq) Cu(NH₃) ₄²⁺(aq)

Correct Answer
verified

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

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, K_c.

Correct Answer
verified

In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant K_c will also increase.

Correct Answer
verified

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

Correct Answer
verified

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X₂(g) + ½Y₂(g) XY(g) (2) 2XY(g) X₂(g) + Y₂(g)

Correct Answer
verified

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Chemical reactions generally reach equilibrium because one of the reactants is used up.

Correct Answer
verified

The following reaction is at equilibrium in a closed container. CuSO₄.5H₂O(s) CuSO₄(s) + 5H₂O(g) Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

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

Correct Answer
verified

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_p = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Correct Answer
verified

Write the mass-action expression, _c, for the following chemical reaction equation. 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

Correct Answer
verified

Exam 17: Equilibrium the Extent of Chemical Reactions

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) ½Br2(g) + ½Cl2(g)

Correct AnswerverifiedShow Answer

H2SO3(aq) HSO3(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction HSO3-(aq) SO32-(aq) + H+(aq) ?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following has an effect on the magnitude of the equilibrium constant?

Correct AnswerverifiedShow Answer

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) NO2(g) (2) 2NO2(g) 2NO(g) + O2(g) Which one of the following is the correct relationship between the equilibrium constants K1 and K2?

Correct AnswerverifiedShow Answer

What is the mass-action expression, c, for the following chemical reaction? Cu2+(aq) + 4NH3(aq) Cu(NH3) 42+(aq)

Correct AnswerverifiedShow Answer

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

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, Kc.

Correct AnswerverifiedShow Answer

In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant Kc will also increase.

Correct AnswerverifiedShow Answer

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g) + Br2(g) 2NOBr(g)

Correct AnswerverifiedShow Answer

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X2(g) + ½Y2(g) XY(g) (2) 2XY(g) X2(g) + Y2(g)

Correct AnswerverifiedShow Answer

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, Kc, will also be doubled.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Chemical reactions generally reach equilibrium because one of the reactants is used up.

Correct AnswerverifiedShow Answer

The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) CuSO4(s) + 5H2O(g) Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?

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

Correct AnswerverifiedShow Answer

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) NH3(g) + HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Correct AnswerverifiedShow Answer

Write the mass-action expression, c, for the following chemical reaction equation. 2C6H6(g) + 15O2(g) 12CO2(g) + 6H2O(g)

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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) ½Br₂(g) + ½Cl₂(g)

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H₂SO₃(aq) HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10^-2 H₂SO₃(aq) SO₃^2-(aq) + 2H⁺(aq) K_c = 9.1 × 10^-10 Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction HSO₃^-(aq) SO₃^2-(aq) + H⁺(aq) ?

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Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) NO2(g) (2) 2NO₂(g) 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

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What is the mass-action expression, c, for the following chemical reaction? Cu₂₊(aq) + 4NH₃(aq) Cu(NH₃) ₄²⁺(aq)

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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.

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Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, K_c.

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In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant K_c will also increase.

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Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

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The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X₂(g) + ½Y₂(g) XY(g) (2) 2XY(g) X₂(g) + Y₂(g)

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If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

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The following reaction is at equilibrium in a closed container. CuSO₄.5H₂O(s) CuSO₄(s) + 5H₂O(g) Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

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

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Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_p = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

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Write the mass-action expression, _c, for the following chemical reaction equation. 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

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