Question 1

A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following reaction: NH4NO3(s)  4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following reaction: NH4NO3(s)    N2O(g)  + 2H2O(g)  At equilibrium, the total pressure in the container was found to be 2.25 atm at a temperature of 500°C. Calculate Kp. A)  2.25. B)  5.06 C)  45.6 D)  1.69 E)  2.25 " class="answers-bank-image d-inline" rel="preload" > N2O(g)  + 2H2O(g) 
At equilibrium, the total pressure in the container was found to be 2.25 atm at a temperature of 500°C. Calculate Kp.

Accepted Answer

A)   2.25.
B)   5.06
C)   45.6
D)   1.69
E)   2.25

Question 2

At a given temperature, the equilibrium constant K for the reaction 2SO2(g)  + O2(g)  2(g)  + O2(g)    2SO3(g)  Is 3.0  109. If 2.60 mol of SO2 and 3.90 mol of O2 are placed in a 1.78-L container and allowed to react to equilibrium at this temperature, what is the concentration of SO3 at equilibrium? A)  1.46 M B)  0.730 M C)  2.92 M D)  3.65 M E)  2.19 M " class="answers-bank-image d-inline" rel="preload" > 2SO3(g) 
Is 3.0  109. If 2.60 mol of SO2 and 3.90 mol of O2 are placed in a 1.78-L container and allowed to react to equilibrium at this temperature, what is the concentration of SO3 at equilibrium?

Accepted Answer

A)   1.46 M
B)   0.730 M
C)   2.92 M
D)   3.65 M
E)   2.19 M

Question 3

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 *10

Question 4

At a certain temperature, K for the reaction 2NO2 2   N2O4 Is 7.5 L/mol. If 2.0 mol of NO2 is placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N2O4 at equilibrium. A)  0.39 mol/L B)  0.82 mol/L C)  7.5 mol/L D)  0.65 mol/L E)  none of these " class="answers-bank-image d-inline" rel="preload" > N2O4
Is 7.5 L/mol. If 2.0 mol of NO2 is placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N2O4 at equilibrium.

Accepted Answer

A)   0.39 mol/L
B)   0.82 mol/L
C)   7.5 mol/L
D)   0.65 mol/L
E)   none of these

Question 5

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 6

What is the value of Q0, the reaction quotient, based on the conditions above?

Accepted Answer

A)   0.50
B)   0.125
C)   4.00
D)   1.00
E)   None of the above

Question 7

The reaction H2(g)  + I2(g)  2(g)  + I2(g)    2HI(g)  Has Kp = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.30 atm and hydrogen gas at a partial pressure of 0.225 atm. What is the partial pressure of I2? A)  1.79 atm B)  0.225 atm C)  0.833 atm D)  37.1 atm E)  0.416 atm " class="answers-bank-image d-inline" rel="preload" > 2HI(g) 
Has Kp = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.30 atm and hydrogen gas at a partial pressure of 0.225 atm. What is the partial pressure of I2?

Accepted Answer

A)   1.79 atm
B)   0.225 atm
C)   0.833 atm
D)   37.1 atm
E)   0.416 atm

Question 8

To achieve equilibrium, the original reaction mixture will

Accepted Answer

A)   produce more water and oxygen only
B)   experience no change in component pressures
C)   always move in a direction to lower the total pressure
D)   shift toward products
E)   shift toward reactants

Question 9

Once equilibrium was established, some additional chlorine gas was added to the system. This resulted in

Accepted Answer

A)   no net change in the amounts of the other reaction components.
B)   an increase in the amount of H2O relative to the equilibrium mixture.
C)   a decrease in the amount of H2O relative to the equilibrium mixture.
D)   a decrease in the amount of HCl relative to the equilibrium mixture.
E)   both B and D

Question 10

Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g)  + O2(g)  2(g)  + O2(g)    2NO(g)  is 0.01. Predict the direction in which the system will move to reach equilibrium at 2000°C if 0.4 mol of N2, 0.1 mol of O2, and 0.08 mol of NO are placed in a 1.0-L container. A)  The system remains unchanged. B)  The concentration of NO will decrease; the concentrations of N2 and O2 will remain unchanged. C)  The concentration of NO will decrease; the concentrations of N2 and O2 will increase. D)  The concentration of NO will increase; the concentrations of N2 and O2 will decrease. E)  More information is necessary. " class="answers-bank-image d-inline" rel="preload" > 2NO(g)  is 0.01. Predict the direction in which the system will move to reach equilibrium at 2000°C if 0.4 mol of N2, 0.1 mol of O2, and 0.08 mol of NO are placed in a 1.0-L container.

Accepted Answer

A)   The system remains unchanged.
B)   The concentration of NO will decrease; the concentrations of N2 and O2 will remain unchanged.
C)   The concentration of NO will decrease; the concentrations of N2 and O2 will increase.
D)   The concentration of NO will increase; the concentrations of N2 and O2 will decrease.
E)   More information is necessary.

Question 11

The equilibrium constant for A + 2B  10-6. Determine the equilibrium constant for 4A + 8B   12C. A)  1.0  10-24 B)  1.0  1024 C)  1.0  10-6 D)  4  10-24 E)  4  10-6 " class="answers-bank-image d-inline" rel="preload" > 3C is 1.0  10-6. Determine the equilibrium constant for 4A + 8B  10-6. Determine the equilibrium constant for 4A + 8B   12C. A)  1.0  10-24 B)  1.0  1024 C)  1.0  10-6 D)  4  10-24 E)  4  10-6 " class="answers-bank-image d-inline" rel="preload" > 12C.

Accepted Answer

A)   1.0  10-24
B)   1.0  1024
C)   1.0  10-6
D)   4  10-24
E)   4  10-6

Exam 6: Chemical Equilibrium

Correct Answer
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At a certain temperature, K for the reaction 2NO₂ N₂O₄ Is 7.5 L/mol. If 2.0 mol of NO₂ is placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N₂O₄ at equilibrium.

Correct Answer
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What is the value of Q₀, the reaction quotient, based on the conditions above?

Correct Answer
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Once equilibrium was established, some additional chlorine gas was added to the system. This resulted in

Correct Answer
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To achieve equilibrium, the original reaction mixture will

Correct Answer
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Which of the following statements concerning equilibrium is not true?

Correct Answer
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At a given temperature, the equilibrium constant K for the reaction 2SO₂(g) + O₂(g) 2SO₃(g) Is 3.0  10⁹. If 2.60 mol of SO₂ and 3.90 mol of O₂ are placed in a 1.78-L container and allowed to react to equilibrium at this temperature, what is the concentration of SO₃ at equilibrium?

Correct Answer
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The equilibrium constant for A + 2B 3C is 1.0  10^-⁶. Determine the equilibrium constant for 4A + 8B 12C.

Correct Answer
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Correct Answer
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The reaction H₂(g) + I₂(g) 2HI(g) Has K_p = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.30 atm and hydrogen gas at a partial pressure of 0.225 atm. What is the partial pressure of I₂?

Correct Answer
verified

Correct Answer
verified
For O₃, 1.3 *10
View Answer

Exam 6: Chemical Equilibrium

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At a certain temperature, K for the reaction 2NO2 N2O4 Is 7.5 L/mol. If 2.0 mol of NO2 is placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N2O4 at equilibrium.

Correct AnswerverifiedShow Answer

What is the value of Q0, the reaction quotient, based on the conditions above?

Correct AnswerverifiedShow Answer

Once equilibrium was established, some additional chlorine gas was added to the system. This resulted in

Correct AnswerverifiedShow Answer

To achieve equilibrium, the original reaction mixture will

Correct AnswerverifiedShow Answer

Which of the following statements concerning equilibrium is not true?

Correct AnswerverifiedShow Answer

At a given temperature, the equilibrium constant K for the reaction 2SO2(g) + O2(g) 2SO3(g) Is 3.0  109. If 2.60 mol of SO2 and 3.90 mol of O2 are placed in a 1.78-L container and allowed to react to equilibrium at this temperature, what is the concentration of SO3 at equilibrium?

Correct AnswerverifiedShow Answer

The equilibrium constant for A + 2B 3C is 1.0  10-6. Determine the equilibrium constant for 4A + 8B 12C.

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A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following reaction: NH4NO3(s) N2O(g) + 2H2O(g) At equilibrium, the total pressure in the container was found to be 2.25 atm at a temperature of 500°C. Calculate Kp.

Correct AnswerverifiedShow Answer

The reaction H2(g) + I2(g) 2HI(g) Has Kp = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.30 atm and hydrogen gas at a partial pressure of 0.225 atm. What is the partial pressure of I2?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedFor O3, 1.3 *10View AnswerShow Answer

Correct Answer
verified

At a certain temperature, K for the reaction 2NO₂ N₂O₄ Is 7.5 L/mol. If 2.0 mol of NO₂ is placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N₂O₄ at equilibrium.

Correct Answer
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What is the value of Q₀, the reaction quotient, based on the conditions above?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

At a given temperature, the equilibrium constant K for the reaction 2SO₂(g) + O₂(g) 2SO₃(g) Is 3.0  10⁹. If 2.60 mol of SO₂ and 3.90 mol of O₂ are placed in a 1.78-L container and allowed to react to equilibrium at this temperature, what is the concentration of SO₃ at equilibrium?

Correct Answer
verified

The equilibrium constant for A + 2B 3C is 1.0  10^-⁶. Determine the equilibrium constant for 4A + 8B 12C.

Correct Answer
verified

Correct Answer
verified

The reaction H₂(g) + I₂(g) 2HI(g) Has K_p = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.30 atm and hydrogen gas at a partial pressure of 0.225 atm. What is the partial pressure of I₂?

Correct Answer
verified

Correct Answer
verified
For O₃, 1.3 *10
View Answer