Question 1

Consider the following equilibrium:
4NH3(g) + 3O2(g) ⇌ 2N2(g) + 6H2O(g) + 1531 kJ
The concentrations of the products will increase when the temperature is increased.

Accepted Answer

A) True 
 B)False

Question 2

Consider the reaction N2(g)  + O2(g)   ⇌\rightleftharpoons⇌  2NO(g) , for which Kc = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, determine the equilibrium concentration of NO.

Accepted Answer

A)   5.4 * 10-3 M
B)   0.0096 M
C)   0.013 M
D)   0.080 M
E)   0.10 M F) A) and E)
G) None of the above

Question 3

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g)  + 1/2O2(g)   ⇌\rightleftharpoons⇌  COCl2(g)  + Cl2(g) , Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g)  + O2(g)   ⇌\rightleftharpoons⇌  2COCl2(g)  + 2Cl2(g) .

Accepted Answer

A)   4.4 * 109
B)   8.8 * 109
C)   1.9 * 1010
D)   1.9 * 1019
E)   2.3 * 10-10 F) A) and D)
G) D) and E)

Question 4

Consider the chemical reaction 2NH3(g)  ⇌ N2(g)  + 3H2(g) . The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)  are present. Estimate the equilibrium concentration of H2(g) .

Accepted Answer

A)   10 M
B)   20 M
C)   30 M
D)   40 M
E)   None of the aboveF) C) and D)
G) A) and E)

Question 5

Consider the following reactions and their associated equilibrium constants:  A+2 B⇋C K1C⇋D+E K2\begin{array}{ll}\mathrm{A}+2 \mathrm{~B} \leftrightharpoons \mathrm{C} & \mathrm{~K}_{1} \\mathrm{C} \leftrightharpoons \mathrm{D}+\mathrm{E} & \mathrm{~K}_{2}\end{array}A+2 B⇋CC⇋D+E​ K1​ K2​​  For the reaction A + 2B (⇌)  D + E, having equilibrium constant Kc,

Accepted Answer

A)   Kc = K1 + K2
B)   Kc = K1/K2
C)   Kc = K1 - K2
D)   Kc = (K1) (K2) 
E)   Kc = K2/K1 F) All of the above
G) None of the above

Question 6

For the reaction 2NOCl(g)  ⇌ 2NO(g)  + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

Accepted Answer

A)   1.26 M
B)   2.25 M
C)   2.50 M
D)   3.52 M
E)   11.0 MF) None of the above
G) D) and E)

Question 7

The common allotropes of carbon (graphite and diamond)  equilibrate as follows: C(gr)  ⇌ C(dia)  with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm3/mol and 3.42 cm3/mol;  Δ\DeltaΔ Hf of diamond is 1.90 kJ/mol. This data suggests that the formation of diamond is favored at

Accepted Answer

A)   low temperatures and low pressures
B)   high temperatures and low pressures
C)   low temperatures and high pressures.
D)   high temperatures and high pressures. E) All of the above
F) B) and C)

Question 8

For the reaction H2(g)  + I2(g)  ⇌ 2HI(g) , Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which of the following is true based on the above

Accepted Answer

A)   Qc > Kc, the reaction proceeds from left to right to reach equilibrium
B)   Qc > Kc, the reaction proceeds from right to left to reach equilibrium
C)   Qc c, the reaction proceeds from left to right to reach equilibrium
D)   Qc c, the reaction proceeds from right to left to reach equilibrium
E)   Qc = Kc, the reaction is currently at equilibriumF) A) and E)
G) B) and D)

Question 9

Consider this gas phase equilibrium system: PCl5(g)  ⇌ PCl3(g)  + Cl2(g)   Δ\DeltaΔ Hºrxn = +87.8 kJ/mol.Which of these statements is false

Accepted Answer

A)   Increasing the system volume shifts the equilibrium to the right.
B)   Increasing the temperature shifts the equilibrium to the right.
C)   A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right.
D)   Decreasing the total pressure of the system shifts the equilibrium to the right.
E)   Increasing the temperature causes the equilibrium constant to increase. F) A) and D)
G) B) and C)

Question 10

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left
2NOBr(g)  ⇌ 2NO(g)  + Br2(g) ,  Δ\DeltaΔ Hºrxn = 30 kJ/mol

Accepted Answer

A)   Increase the container volume.
B)   Remove some NO.
C)  Remove some Br2.
D)   Add more NOBr.
E)   Decrease the temperature. F) A) and E)
G) A) and D)

Question 11

For the reaction SO2(g)  + NO2(g)   ⇌\rightleftharpoons⇌  SO3(g)  + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium

Accepted Answer

A)   0.48 mol/L
B)   0.11 mol/L
C)   0.95 mol/L
D)   2.22 mol/L
E)   18 mol/L F) A) and B)
G) B) and E)

Question 12

What is the correct equilibrium constant expression for this reaction
2HI(g)  ⇌ H2(g)  + I2(g)

Accepted Answer

A)   Kc = [H2] [I2]/[HI]
B)   Kc = [HI]2/[H2] [I2]
C)   Kc = [HI] /[H2] [I2]
D)   Kc = [H2] [I2]/[HI]2
E)   None of the aboveF) A) and B)
G) B) and D)

Question 13

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

Accepted Answer

A) True 
 B)False

Question 14

The equilibrium constant for the chemical equation
2NO(g) + O2(g) ⇌ 2NO2(g)
is two times the equilibrium constant for the chemical equation
NO(g) + 1/2O2(g) ⇌ NO2(g).

Accepted Answer

A) True 
 B)False

Question 15

At 700 K, the reaction 2SO2(g)  + O2(g)  ⇌ 2SO3(g)  has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Which of the following is true based on the above

Accepted Answer

A)   Qc > Kc, the reaction proceeds from left to right to reach equilibrium
B)   Qc > Kc, the reaction proceeds from right to left to reach equilibrium
C)   Qc c, the reaction proceeds from left to right to reach equilibrium
D)   Qc c, the reaction proceeds from right to left to reach equilibrium
E)   Qc = Kc, the reaction is currently at equilibriumF) C) and D)
G) A) and C)

Question 16

For the reaction at equilibrium: CO(g)  + H2O(g)  ⇌ CO2(g)  + H2(g) , increasing the volume of the container would:

Accepted Answer

A)   Shift the equilibrium to the right
B)   Shift the equilibrium to the left
C)   Increase the value of the equilibrium constant, K
D)   Decrease the value of the equilibrium constant, K
E)   Cause no changeF) B) and E)
G) None of the above

Question 17

Calculate Kc for the reaction 2HI(g)   ⇌\rightleftharpoons⇌  H2(g)  + I2(g)  given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Accepted Answer

A)   5.25
B)   0.22
C)   4.5
D)   0.19
E)   1.6 * 102 F) B) and E)
G) C) and D)

Question 18

For the reaction PCl3(g)  + Cl2(g)  ⇌ PCl5(g)  at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of the following is true based on the above

Accepted Answer

A)   Qc > Kc, the reaction proceeds from left to right to reach equilibrium
B)   Qc > Kc, the reaction proceeds from right to left to reach equilibrium
C)   Qc c, the reaction proceeds from left to right to reach equilibrium
D)   Qc c, the reaction proceeds from right to left to reach equilibrium
E)   Qc = Kc, the reaction is currently at equilibriumF) D) and E)
G) A) and E)

Question 19

Concerning the following reaction at equilibrium: 3Fe(s)  + 4H2O(g)  ⇌ Fe3O4(s)  + 4H2(g) , increasing the volume of the container would:

Accepted Answer

A)   Shift the equilibrium to the right
B)   Shift the equilibrium to the left
C)   Increase the value of the equilibrium constant, K
D)   Decrease the value of the equilibrium constant, K
E)   Cause no changeF) None of the above
G) D) and E)

Question 20

The Kc for the reaction CO2(g)  + H2(g)  ⇌ H2O(g)  + CO(g)  is 1.6 at about 990ºC. Calculate the number of moles of water in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Accepted Answer

A)   1.7 mol
B)   1.5 mol
C)   1.3 mol
D)   1.1 mol
E)   None of the aboveF) A) and B)
G) A) and D)

Exam 14: Chemical Equilibrium

What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H₂(g) + I₂(g)

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

Correct Answer
verified

Consider the chemical reaction 2NH₃(g) ⇌ N₂(g) + 3H₂(g) . The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g) are present. Estimate the equilibrium concentration of H₂(g) .

Correct Answer
verified

The K_c for the reaction CO₂(g) + H₂(g) ⇌ H₂O(g) + CO(g) is 1.6 at about 990ºC. Calculate the number of moles of water in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct Answer
verified

Correct Answer
verified

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br₂(g) , $\Delta$ Hº_rxn = 30 kJ/mol

Correct Answer
verified

At 700 K, the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) has the equilibrium constant K_c = 4.3 * 10⁶ , and the following concentrations are present: [SO₂] = 0.10 M; [SO₃] = 10. M; [O₂] = 0.10 M. Which of the following is true based on the above

Correct Answer
verified

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g) , K_c = 50.2 at 445ºC. If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which of the following is true based on the above

Correct Answer
verified

For the reaction at equilibrium: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) , increasing the volume of the container would:

Correct Answer
verified

Consider the following equilibrium: 4NH₃(g) + 3O₂(g) ⇌ 2N₂(g) + 6H₂O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) at a particular temperature, K_c = 24.3. Suppose a system at that temperature is prepared with [PCl₃] = 0.10 M, [Cl₂] = 0.15 M, and [PCl₅] = 0.60 M. Which of the following is true based on the above

Correct Answer
verified

Consider this gas phase equilibrium system: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) $\Delta$ Hº_rxn = +87.8 kJ/mol.Which of these statements is false

Correct Answer
verified

Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g) , increasing the volume of the container would:

Correct Answer
verified

For the reaction 2NOCl(g) ⇌ 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

Correct Answer
verified

The equilibrium constant for the chemical equation 2NO(g) + O₂(g) ⇌ 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g) + ¹/₂O₂(g) ⇌ NO₂(g).

Correct Answer
verified

Correct Answer
verified

For the reaction SO₂(g) + NO₂(g) $\rightleftharpoons$ SO₃(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20. L container, what concentration of SO₃ will be present at equilibrium

Correct Answer
verified

Consider the reaction N₂(g) + O₂(g) $\rightleftharpoons$ 2NO(g) , for which K_c = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

Correct Answer
verified

Exam 14: Chemical Equilibrium

What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H2(g) + I2(g)

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Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

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Consider the chemical reaction 2NH3(g) ⇌ N2(g) + 3H2(g) . The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g) are present. Estimate the equilibrium concentration of H2(g) .

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The Kc for the reaction CO2(g) + H2(g) ⇌ H2O(g) + CO(g) is 1.6 at about 990ºC. Calculate the number of moles of water in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

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Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) ⇌\rightleftharpoons⇌ COCl2(g) + Cl2(g) , Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g) ⇌\rightleftharpoons⇌ 2COCl2(g) + 2Cl2(g) .

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For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br2(g) , Δ\DeltaΔ Hºrxn = 30 kJ/mol

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At 700 K, the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Which of the following is true based on the above

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For the reaction H2(g) + I2(g) ⇌ 2HI(g) , Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which of the following is true based on the above

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For the reaction at equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) , increasing the volume of the container would:

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Consider the following equilibrium: 4NH3(g) + 3O2(g) ⇌ 2N2(g) + 6H2O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.

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Calculate Kc for the reaction 2HI(g) ⇌\rightleftharpoons⇌ H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

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For the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of the following is true based on the above

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Consider this gas phase equilibrium system: PCl5(g) ⇌ PCl3(g) + Cl2(g) Δ\DeltaΔ Hºrxn = +87.8 kJ/mol.Which of these statements is false

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Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g) , increasing the volume of the container would:

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For the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

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The equilibrium constant for the chemical equation 2NO(g) + O2(g) ⇌ 2NO2(g) is two times the equilibrium constant for the chemical equation NO(g) + 1/2O2(g) ⇌ NO2(g).

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For the reaction SO2(g) + NO2(g) ⇌\rightleftharpoons⇌ SO3(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium

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Consider the reaction N2(g) + O2(g) ⇌\rightleftharpoons⇌ 2NO(g) , for which Kc = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, determine the equilibrium concentration of NO.

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What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H₂(g) + I₂(g)

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

Correct Answer
verified

Consider the chemical reaction 2NH₃(g) ⇌ N₂(g) + 3H₂(g) . The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g) are present. Estimate the equilibrium concentration of H₂(g) .

Correct Answer
verified

The K_c for the reaction CO₂(g) + H₂(g) ⇌ H₂O(g) + CO(g) is 1.6 at about 990ºC. Calculate the number of moles of water in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct Answer
verified

Correct Answer
verified

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br₂(g) , $\Delta$ Hº_rxn = 30 kJ/mol

Correct Answer
verified

At 700 K, the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) has the equilibrium constant K_c = 4.3 * 10⁶ , and the following concentrations are present: [SO₂] = 0.10 M; [SO₃] = 10. M; [O₂] = 0.10 M. Which of the following is true based on the above

Correct Answer
verified

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g) , K_c = 50.2 at 445ºC. If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which of the following is true based on the above

Correct Answer
verified

For the reaction at equilibrium: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) , increasing the volume of the container would:

Correct Answer
verified

Consider the following equilibrium: 4NH₃(g) + 3O₂(g) ⇌ 2N₂(g) + 6H₂O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) at a particular temperature, K_c = 24.3. Suppose a system at that temperature is prepared with [PCl₃] = 0.10 M, [Cl₂] = 0.15 M, and [PCl₅] = 0.60 M. Which of the following is true based on the above

Correct Answer
verified

Consider this gas phase equilibrium system: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) $\Delta$ Hº_rxn = +87.8 kJ/mol.Which of these statements is false

Correct Answer
verified

Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g) , increasing the volume of the container would:

Correct Answer
verified

For the reaction 2NOCl(g) ⇌ 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

Correct Answer
verified

The equilibrium constant for the chemical equation 2NO(g) + O₂(g) ⇌ 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g) + ¹/₂O₂(g) ⇌ NO₂(g).

Correct Answer
verified

Correct Answer
verified

For the reaction SO₂(g) + NO₂(g) $\rightleftharpoons$ SO₃(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20. L container, what concentration of SO₃ will be present at equilibrium

Correct Answer
verified

Consider the reaction N₂(g) + O₂(g) $\rightleftharpoons$ 2NO(g) , for which K_c = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

Correct Answer
verified