Question 1

For the reaction 2H2(g)  + O2(g)  2(g)  + O2(g)    2H2O(g) , what is the relationship between K and Kp at temperature T? A)  Kp = K(RT) 2 B)  K = Kp(RT)  C)  K = Kp D)  Kp = K(RT)  E)  K = Kp(RT) 2" class="answers-bank-image d-inline" rel="preload" > 2H2O(g) , what is the relationship between K and Kp at temperature T?

Accepted Answer

A)   Kp = K(RT) 2
B)   K = Kp(RT) 
C)   K = Kp
D)   Kp = K(RT) 
E)   K = Kp(RT) 2

Question 2

Consider the equation 2A(g)  4. -Addition of chemical B to an equilibrium mixture of the above will A)  cause [A] to increase. B)  have no effect. C)  cause [C] to increase. D)  cannot be determined E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2B(g)  + C(g) . At a particular temperature, K = 1.6 × 104.
-Addition of chemical B to an equilibrium mixture of the above will

Accepted Answer

A)   cause [A] to increase.
B)   have no effect.
C)   cause [C] to increase.
D)   cannot be determined
E)   none of these

Question 3

Consider the following equilibrium:N2(g)  + 3H2(g)  2(g)  + 3H2(g)    2NH3(g)  with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H2. A)  0.5 M B)  1.0 M C)  2.5 M D)  2.0 M E)  1.5 M" class="answers-bank-image d-inline" rel="preload" > 2NH3(g) 
with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container.
-Calculate the equilibrium concentration of H2.

Accepted Answer

A)   0.5 M
B)   1.0 M
C)   2.5 M
D)   2.0 M
E)   1.5 M

Question 4

Write the equilibrium constant expression for the following reaction:
CaCO3(s)  
CaO(s) + CO2(g)

Accepted Answer

Question 5

Consider the following chemical reaction involving a pure solid sample A that yields products B and C:
3A(s)  
3B(g)  + 2C(g) 
Identify the equilibrium expression of the reaction.​

Accepted Answer

A)   ​ 
B)   ​ 
C)   ​ 
D)   ​ 
E)   ​

Question 6

Consider the equation A(aq)  + 2B(aq)  -4 E)  0.013" class="answers-bank-image d-inline" rel="preload" > 3C(aq)  + 2D(aq) . 40.0 mL of 0.056 M A is mixed with 25.0 mL 0.108 M B. At equilibrium, the concentration of C is 0.0412 M. Calculate K.

Accepted Answer

A)   0.029
B)   2.6
C)   0.0020
D)   1.9 × 10-4
E)   0.013

Question 7

Consider the decomposition of hydrazine as shown below.N2H4(g)  2H4(g)    2H2(g)  + N2(g)  At a certain temperature, Kp = 2.5 × 103. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium. A)  76 atm B)  5776 atm C)  54 atm D)  127 atm E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2H2(g)  + N2(g) 
At a certain temperature, Kp = 2.5 × 103. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium.

Accepted Answer

A)   76 atm
B)   5776 atm
C)   54 atm
D)   127 atm
E)   none of these

Question 8

For the reaction below, Kp = 1.16 at 890.°C.
          CaCO3(s)  ⇌ CaO(s)  + CO2(g) 
If a 22.0-g sample of CaCO3 is put into a 10.4-L container and heated to 890.°C, what percent of the CaCO3 will react to reach equilibrium?

Accepted Answer

A)  12.6%
B)  25.3%
C)  57.5%
D)  100.%
E)   54.9%

Question 9

Consider the following equilibrium:N2(g)  + 3H2(g)  2(g)  + 3H2(g)    2NH3(g)  with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH3(g) . A)  3.7 × 10-3 M B)  5.4 × 10-5 M C)  7.3 × 10-3 M D)  4.3 × 10-6 M E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2NH3(g) 
with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container.
-Calculate the equilibrium concentration of NH3(g) .

Accepted Answer

A)   3.7 × 10-3 M
B)   5.4 × 10-5 M
C)   7.3 × 10-3 M
D)   4.3 × 10-6 M
E)   none of these

Question 10

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products?
CuO(s)  + H2(g)  2(g)    Cu(s)  + H2O(g)  Change in enthalpy = -2.0 kJ. A)  Increase the pressure by adding an inert gas such as nitrogen. B)  Allow some gas to escape at constant pressure and temperature. C)  Decrease the temperature. D)  Increase the pressure by means of a moving piston at constant temperature. E)  Add a catalyst." class="answers-bank-image d-inline" rel="preload" >
Cu(s)  + H2O(g) 
Change in enthalpy = -2.0 kJ.

Accepted Answer

A)   Increase the pressure by adding an inert gas such as nitrogen.
B)   Allow some gas to escape at constant pressure and temperature.
C)   Decrease the temperature.
D)   Increase the pressure by means of a moving piston at constant temperature.
E)   Add a catalyst.

Question 11

The value of the equilibrium constant K is dependent on:
I.the temperature of the system.
II.the nature of the reactants and products.
III.the concentration of the reactants.
IV.the concentration of the products.

Accepted Answer

A)   I and II only
B)   III and IV only
C)   II and III only
D)   three of these
E)   none of these

Question 12

Consider the following reaction, which is involved in the catalytic destruction of ozone by chlorine atoms.
ClO(g) + O3(g)  Cl(g) + 2O2(g)
Kp = 2.5 × 106 atm at 25° C. In an experiment at 25° C, ClO(g) at 1.0 × 10-3 atm was mixed with O3(g) at 2.0 ×10-5 atm in a rigid vessel. Calculate the equilibrium pressure of O3(g) and O2(g).

Accepted Answer

For O₃, 1.3...

Question 13

In the reaction
P4(g) 2P2(g)Kp = 0.500 atm at 1052°C.
 In an experiment, P4(g) is initially placed into a container at 1052°C. The total pressure of the equilibrium mixture of P4(g) and P2(g) is 6.00 atm. Calculate the equilibrium pressures of P4(g) and P2(g). Calculate the fraction (by moles) of P4(g) that has dissociated to reach equilibrium.

Accepted Answer

Pressure of P₄ = 4.50...

Question 14

Which of the following statements concerning equilibrium is not true?

Accepted Answer

A)   A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium.
B)   The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained.
C)   Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another.
D)   The equilibrium constant is independent of temperature.
E)   A system moves spontaneously toward a state of equilibrium.

Question 15

Which of the following statements is false?

Accepted Answer

A)   Decreasing the volume of the container shifts the equilibrium to form more PCl5.
B)   Removing PCl5 from the container shifts the equilibrium to form more PCl3.
C)   Adding PCl3 to the container shifts the equilibrium to form more PCl5.
D)   Increasing the temperature shifts the equilibrium to form more PCl3.

Question 16

For the hypothetical reactions 1 and 2, K1 = 102 and K2 = 10-4.
1)  A2(g)  + B2(g)  1 = 102 and K2 = 10-4. 1)  A2(g)  + B2(g)    2AB(g)  2)  2A2(g)  + C2(g)   2A2C(g)  3)  A2C(g)  + B2(g)   2AB(g)  + (1/2) C2(g)  What is the value for K for reaction 3? A)  10-2 B)  104 C)  106 D)  102 E)  10-4" class="answers-bank-image d-inline" rel="preload" > 2AB(g) 
2)  2A2(g)  + C2(g)  1 = 102 and K2 = 10-4. 1)  A2(g)  + B2(g)    2AB(g)  2)  2A2(g)  + C2(g)   2A2C(g)  3)  A2C(g)  + B2(g)   2AB(g)  + (1/2) C2(g)  What is the value for K for reaction 3? A)  10-2 B)  104 C)  106 D)  102 E)  10-4" class="answers-bank-image d-inline" rel="preload" >2A2C(g) 
3)  A2C(g)  + B2(g)  1 = 102 and K2 = 10-4. 1)  A2(g)  + B2(g)    2AB(g)  2)  2A2(g)  + C2(g)   2A2C(g)  3)  A2C(g)  + B2(g)   2AB(g)  + (1/2) C2(g)  What is the value for K for reaction 3? A)  10-2 B)  104 C)  106 D)  102 E)  10-4" class="answers-bank-image d-inline" rel="preload" >2AB(g)  + (1/2) C2(g) 
What is the value for K for reaction 3?

Accepted Answer

A)   10-2
B)   104
C)   106
D)   102
E)   10-4

Question 17

Consider the equation 2A(g)  4.At a higher temperature, K = 1.8 × 10-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C. A)  2.6 × 10-2 M B)  6.0 × 10-3 M C)  1.0 M D)  2.1 × 10-2 M E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2B(g)  + C(g) . At a particular temperature, K = 1.6 × 104.At a higher temperature, K = 1.8 × 10-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C.

Accepted Answer

A)   2.6 × 10-2 M
B)   6.0 × 10-3 M
C)   1.0 M
D)   2.1 × 10-2 M
E)   none of these

Question 18

Consider the equation 2A(g)  4.Placing the equilibrium mixture in an ice bath (thus lowering the temperature)  will A)  have no effect. B)  cause [A] to increase. C)  cause [B] to increase. D)  cannot be determined E)  none of these " class="answers-bank-image d-inline" rel="preload" > 2B(g)  + C(g) . At a particular temperature, K = 1.6 × 104.Placing the equilibrium mixture in an ice bath (thus lowering the temperature)  will

Accepted Answer

A)   have no effect.
B)   cause [A] to increase.
C)   cause [B] to increase.
D)   cannot be determined
E)   none of these

Exam 6: Chemical Equilibrium

Which of the following statements concerning equilibrium is not true?

Correct Answer
verified

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H₂(g) Cu(s) + H₂O(g) Change in enthalpy = -2.0 kJ.

Correct Answer
verified

Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq) . 40.0 mL of 0.056 M A is mixed with 25.0 mL 0.108 M B. At equilibrium, the concentration of C is 0.0412 M. Calculate K.

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴. -Addition of chemical B to an equilibrium mixture of the above will

Correct Answer
verified

For the hypothetical reactions 1 and 2, K₁ = 10² and K₂ = 10^-4. 1) A₂(g) + B₂(g) 2AB(g) 2) 2A₂(g) + C₂(g) 2A₂C(g) 3) A₂C(g) + B₂(g) 2AB(g) + (1/2) C₂(g) What is the value for K for reaction 3?

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴.Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will

Correct Answer
verified

Consider the following equilibrium:N₂(g) + 3H₂(g) 2NH₃(g) with K = 2.3 × 10^-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H₂.

Correct Answer
verified

For the reaction 2H₂(g) + O₂(g) 2H₂O(g) , what is the relationship between K and K_p at temperature T?

Correct Answer
verified

Write the equilibrium constant expression for the following reaction: CaCO₃(s) CaO(s) + CO₂(g)

Correct Answer
verified

Correct Answer
verified
Pressure of P₄ = 4.50...
View Answer

Correct Answer
verified
For O₃, 1.3...
View Answer

The value of the equilibrium constant K is dependent on: I.the temperature of the system. II.the nature of the reactants and products. III.the concentration of the reactants. IV.the concentration of the products.

Correct Answer
verified

Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.

Correct Answer
verified

Correct Answer
verified

Consider the following equilibrium:N₂(g) + 3H₂(g) 2NH₃(g) with K = 2.3 × 10^-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH₃(g) .

Correct Answer
verified

For the reaction below, Kp = 1.16 at 890.°C. CaCO₃(s) ⇌ CaO(s) + CO₂(g) If a 22.0-g sample of CaCO₃ is put into a 10.4-L container and heated to 890.°C, what percent of the CaCO₃ will react to reach equilibrium?

Correct Answer
verified

Which of the following statements is false?

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴.At a higher temperature, K = 1.8 × 10^-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C.

Correct Answer
verified

Exam 6: Chemical Equilibrium

Which of the following statements concerning equilibrium is not true?

Correct AnswerverifiedShow Answer

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H2(g) Cu(s) + H2O(g) Change in enthalpy = -2.0 kJ.

Correct AnswerverifiedShow Answer

Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq) . 40.0 mL of 0.056 M A is mixed with 25.0 mL 0.108 M B. At equilibrium, the concentration of C is 0.0412 M. Calculate K.

Correct AnswerverifiedShow Answer

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104. -Addition of chemical B to an equilibrium mixture of the above will

Correct AnswerverifiedShow Answer

For the hypothetical reactions 1 and 2, K1 = 102 and K2 = 10-4. 1) A2(g) + B2(g) 2AB(g) 2) 2A2(g) + C2(g) 2A2C(g) 3) A2C(g) + B2(g) 2AB(g) + (1/2) C2(g) What is the value for K for reaction 3?

Correct AnswerverifiedShow Answer

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104.Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will

Correct AnswerverifiedShow Answer

Consider the following equilibrium:N2(g) + 3H2(g) 2NH3(g) with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H2.

Correct AnswerverifiedShow Answer

For the reaction 2H2(g) + O2(g) 2H2O(g) , what is the relationship between K and Kp at temperature T?

Correct AnswerverifiedShow Answer

Write the equilibrium constant expression for the following reaction: CaCO3(s) CaO(s) + CO2(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedPressure of P4 = 4.50...View AnswerShow Answer

Correct AnswerverifiedFor O3, 1.3...View AnswerShow Answer

The value of the equilibrium constant K is dependent on: I.the temperature of the system. II.the nature of the reactants and products. III.the concentration of the reactants. IV.the concentration of the products.

Correct AnswerverifiedShow Answer

Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the following equilibrium:N2(g) + 3H2(g) 2NH3(g) with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH3(g) .

Correct AnswerverifiedShow Answer

For the reaction below, Kp = 1.16 at 890.°C. CaCO3(s) ⇌ CaO(s) + CO2(g) If a 22.0-g sample of CaCO3 is put into a 10.4-L container and heated to 890.°C, what percent of the CaCO3 will react to reach equilibrium?

Correct AnswerverifiedShow Answer

Which of the following statements is false?

Correct AnswerverifiedShow Answer

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104.At a higher temperature, K = 1.8 × 10-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C.

Correct AnswerverifiedShow Answer

Correct Answer
verified

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H₂(g) Cu(s) + H₂O(g) Change in enthalpy = -2.0 kJ.

Correct Answer
verified

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴. -Addition of chemical B to an equilibrium mixture of the above will

Correct Answer
verified

For the hypothetical reactions 1 and 2, K₁ = 10² and K₂ = 10^-4. 1) A₂(g) + B₂(g) 2AB(g) 2) 2A₂(g) + C₂(g) 2A₂C(g) 3) A₂C(g) + B₂(g) 2AB(g) + (1/2) C₂(g) What is the value for K for reaction 3?

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴.Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will

Correct Answer
verified

Consider the following equilibrium:N₂(g) + 3H₂(g) 2NH₃(g) with K = 2.3 × 10^-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H₂.

Correct Answer
verified

For the reaction 2H₂(g) + O₂(g) 2H₂O(g) , what is the relationship between K and K_p at temperature T?

Correct Answer
verified

Write the equilibrium constant expression for the following reaction: CaCO₃(s) CaO(s) + CO₂(g)

Correct Answer
verified

Correct Answer
verified
Pressure of P₄ = 4.50...
View Answer

Correct Answer
verified
For O₃, 1.3...
View Answer

Correct Answer
verified

Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.

Correct Answer
verified

Correct Answer
verified

Consider the following equilibrium:N₂(g) + 3H₂(g) 2NH₃(g) with K = 2.3 × 10^-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH₃(g) .

Correct Answer
verified

For the reaction below, Kp = 1.16 at 890.°C. CaCO₃(s) ⇌ CaO(s) + CO₂(g) If a 22.0-g sample of CaCO₃ is put into a 10.4-L container and heated to 890.°C, what percent of the CaCO₃ will react to reach equilibrium?

Correct Answer
verified

Correct Answer
verified

Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10⁴.At a higher temperature, K = 1.8 × 10^-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C.

Correct Answer
verified