Question 1

Kp for the reaction 4CuO(s)   ⇌\rightleftharpoons⇌  2Cu2O(s)  + O2(g)  is 0.49 at 1024 ∘\circ∘ C. Calculate Kc at this temperature

Accepted Answer

A)   5.8 x 10-3
B)   41
C)   52
D)   4.6 x 10-3
E)   0.49 F) B) and D)
G) A) and B)

Question 2

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When nitrogen is removed from the system at equilibrium, the hydrogen (H2) concentration will increase.

Accepted Answer

A) True 
 B)False

Question 3

Hydrogen iodide decomposes according to the equation: 2HI(g)  ⇌ H2(g)  + I2(g) , Kc = 0.0156 at 400ºC
a 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.Calculate the concentration of HI at equilibrium.

Accepted Answer

A)   0.264 M
B)   0.244 M
C)   0.224 M
D)   0.204 M
E)   None of the aboveF) A) and B)
G) B) and E)

Question 4

For the reaction H2(g) + I2(g) ⇌ 2HI(g), KP = Kc.

Accepted Answer

A) True 
 B)False

Question 5

At 250ºC, the equilibrium constant Kp for the reaction PCl5(g)   ⇌\rightleftharpoons⇌  PCl3(g)  + Cl2(g)  is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium.

Accepted Answer

A)   1.50 atm
B)   1.24 atm
C)   4.24 atm
D)   0.94 atm
E)   1.12 atm F) C) and E)
G) A) and B)

Question 6

The equilibrium constant for the reaction Ni(s)  + 4CO(g)   ⇌\rightleftharpoons⇌  Ni(CO) 4(g)  is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO) 4(g)   ⇌\rightleftharpoons⇌   Ni(s)  + 4CO(g)

Accepted Answer

A)   2.0 * 10-5
B)   2.5 * 109
C)   5.0 * 104
D)   5.0 * 10-4
E)   2.0 * 10-3 F) A) and E)
G) B) and D)

Question 7

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide as shown below.CaCO3(s)  ⇌ CaO(s)  + CO2(g)  The KP for this reaction is 1.16 at 800 ∘\circ∘ C. A 5.00 L vessel containing 10.0 g of CaCO3(s)  was evacuated to remove the air, sealed, and then heated to 800 ∘\circ∘ C. Ignoring the volume occupied by the solid, what will be the overall mass percent of carbon in the solid once equilibrium is reached

Accepted Answer

A)   5.36% carbon by mass
B)   5.56% carbon by mass
C)   5.76% carbon by mass
D)   5.96% carbon by mass
E)   None of the above F) C) and D)
G) D) and E)

Question 8

The following data for the reaction:
A(g) + 2B(s) ⇌ AB2(g) provides evidence that the reaction is exothermic. 
 
 $\begin{array}{|l|l|}
\hline \text { Temperature }(\mathrm{K}) & \mathrm{K}_{\mathrm{c}} \
\hline 300 & 1.5 \times 10^{4} \
\hline 600 & 55 \
\hline 900 & 3.4 \times 10^{-3} \
\hline
\end{array}$

Accepted Answer

A) True 
 B)False

Question 9

For the reaction at equilibrium 2SO3 ⇌ 2SO2 + O2 ( Δ\DeltaΔ Hºrxn= 198 kJ/mol) , increasing the reaction temperature would:

Accepted Answer

A)   Shift the equilibrium to the right and increase the value of the equilibrium constant K
B)   Shift the equilibrium to the left and increase the value of the equilibrium constant K
C)   Shift the equilibrium to the right and decrease the value of the equilibrium constant K
D)   Shift the equilibrium to the left and decrease the value of the equilibrium constant K
E)   Cause no change F) A) and B)
G) A) and C)

Question 10

The conditions used in the Haber process to enhance the yield of ammonia are low pressure and high temperature.

Accepted Answer

A) True 
 B)False

Question 11

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)  + H2(g)  ⇌ H2O(g)  + Cu(s)   Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

Accepted Answer

A)   increasing the pressure by means of a moving piston at constant T.
B)   increasing the pressure by adding an inert gas such as nitrogen.
C)   decreasing the temperature.
D)   allowing some gases to escape at constant P and T.
E)   adding a catalyst. F) A) and D)
G) A) and C)

Question 12

1.25 moles of NOCl were placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g)   ⇌\rightleftharpoons⇌  2NO(g)  + Cl2(g) .

Accepted Answer

A)   3.0 * 10-4
B)   1.8 * 103
C)   1.4 * 10-3
D)   5.6 * 10-4
E)   4.1 * 10-3 F) C) and D)
G) A) and C)

Question 13

75.0 g of PCl5(g)  is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) , and the system is allowed to reach equilibrium at 250ºC.PCl5(g)  ⇌ PCl3(g)  + Cl2(g)  
If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium

Accepted Answer

A)   6.83 atm
B)   8.85 atm
C)   5.38 atm
D)   3.47 atm
E)   7.42 atmF) D) and E)
G) C) and D)

Question 14

For the nitrogen fixation reaction 3H2(g)  + N2(g)  ⇌ 2NH3(g) , Kc = 6.0 * 10-2 at 500 ∘\circ∘ C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2

Accepted Answer

A)   0.750 M
B)   2.7 M
C)   0.250 M
D)   0.025 M
E)   1.85 M F) A) and B)
G) B) and E)

Question 15

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The production of ammonia is an exothermic reaction. When heat is added to the equilibrium system it will shift to increase the amount of ammonia produced.

Accepted Answer

A) True 
 B)False

Question 16

Hydrogen iodide decomposes according to the equation 2HI(g)   ⇌\rightleftharpoons⇌  H2(g)  + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Accepted Answer

A)   0.138 M
B)   0.220 M
C)   0.550 M
D)   0.275 M
E)   0.0275 M F) C) and D)
G) B) and E)

Question 17

Consider this reaction at equilibrium: 2SO2(g)  + O2(g)  ⇌ 2SO3(g) ,  Δ\DeltaΔ Hºrxn = -198 kJ/mol
If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium

Accepted Answer

A)   A shift to produce more SO2
B)   A shift to produce more O2
C)   No change
D)   A shift to produce more SO3 E) B) and D)
F) A) and D)

Question 18

Which is the correct equilibrium constant expression for the following reaction
Fe2O3 (s)  + 3H2 (g)   ⇌\rightleftharpoons⇌  2Fe (s)  + 3H2O (g)

Accepted Answer

A)   Kc = [Fe2O3] [H2]3 / [Fe]2[H2O]3
B)   Kc = [H2] / [H2O]
C)   Kc = [H2O]3 / [H2]3
D)   Kc = [Fe]2[H2O]3 / [Fe2O3] [H2]3
E)   Kc = [Fe] [H2O] / [Fe2O3] [H2] F) A) and D)
G) A) and C)

Question 19

Hydrogen iodide decomposes according to the equation 2HI(g)   ⇌\rightleftharpoons⇌  H2(g)  + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H2 at equilibrium.

Accepted Answer

A)   0.275 M
B)   0.138 M
C)   0.0275 M
D)   0.0550 M
E)   0.220 M F) C) and D)
G) A) and E)

Question 20

Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g)   ⇌\rightleftharpoons⇌  CO(g)  + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

Accepted Answer

A)   0.125
B)   8.0
C)   6.1
D)   0.16
E)   0.083 F) C) and D)
G) B) and E)

Exam 14: Chemical Equilibrium

1.25 moles of NOCl were placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, K_c, for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) .

Correct Answer
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Consider this reaction at equilibrium: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) , $\Delta$ Hº_rxn = -198 kJ/mol If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium

Correct Answer
verified

The conditions used in the Haber process to enhance the yield of ammonia are low pressure and high temperature.

Correct Answer
verified

K_p for the reaction 4CuO(s) $\rightleftharpoons$ 2Cu₂O(s) + O₂(g) is 0.49 at 1024^$\circ$C. Calculate K_c at this temperature

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

Correct Answer
verified

Hydrogen iodide decomposes according to the equation: 2HI(g) ⇌ H₂(g) + I₂(g) , K_c = 0.0156 at 400ºC a 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.Calculate the concentration of HI at equilibrium.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is removed from the system at equilibrium, the hydrogen (H₂) concentration will increase.

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). The production of ammonia is an exothermic reaction. When heat is added to the equilibrium system it will shift to increase the amount of ammonia produced.

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction Fe₂O₃ (s) + 3H₂ (g) $\rightleftharpoons$ 2Fe (s) + 3H₂O (g)

Correct Answer
verified

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) ⇌ H₂O(g) + Cu(s) $\Delta$ Hº_rxn = -2.0 kJ/mol

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) $\rightleftharpoons$ CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

Correct Answer
verified

At 250ºC, the equilibrium constant K_p for the reaction PCl₅(g) $\rightleftharpoons$ PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
verified

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), K_P = K_c.

Correct Answer
verified

75.0 g of PCl₅(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl₂(g) , and the system is allowed to reach equilibrium at 250ºC.PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) If K_p = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium

Correct Answer
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For the reaction at equilibrium 2SO₃ ⇌ 2SO₂ + O₂ ( $\Delta$ Hº_rxn= 198 kJ/mol) , increasing the reaction temperature would:

Correct Answer
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The equilibrium constant for the reaction Ni(s) + 4CO(g) $\rightleftharpoons$ Ni(CO) ₄(g) is 5.0 * 10⁴ at 25ºC. What is the equilibrium constant for the reaction Ni(CO) ₄(g) $\rightleftharpoons$ Ni(s) + 4CO(g)

Correct Answer
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For the nitrogen fixation reaction 3H₂(g) + N₂(g) ⇌ 2NH₃(g) , K_c = 6.0 * 10^-2 at 500^$\circ$C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂

Correct Answer
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Hydrogen iodide decomposes according to the equation 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Correct Answer
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Exam 14: Chemical Equilibrium

1.25 moles of NOCl were placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g) ⇌\rightleftharpoons⇌ 2NO(g) + Cl2(g) .

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Consider this reaction at equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g) , Δ\DeltaΔ Hºrxn = -198 kJ/mol If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium

Correct AnswerverifiedShow Answer

The conditions used in the Haber process to enhance the yield of ammonia are low pressure and high temperature.

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Kp for the reaction 4CuO(s) ⇌\rightleftharpoons⇌ 2Cu2O(s) + O2(g) is 0.49 at 1024 ∘\circ∘ C. Calculate Kc at this temperature

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Hydrogen iodide decomposes according to the equation 2HI(g) ⇌\rightleftharpoons⇌ H2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H2 at equilibrium.

Correct AnswerverifiedShow Answer

Hydrogen iodide decomposes according to the equation: 2HI(g) ⇌ H2(g) + I2(g) , Kc = 0.0156 at 400ºC a 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.Calculate the concentration of HI at equilibrium.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When nitrogen is removed from the system at equilibrium, the hydrogen (H2) concentration will increase.

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Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The production of ammonia is an exothermic reaction. When heat is added to the equilibrium system it will shift to increase the amount of ammonia produced.

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Which is the correct equilibrium constant expression for the following reaction Fe2O3 (s) + 3H2 (g) ⇌\rightleftharpoons⇌ 2Fe (s) + 3H2O (g)

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When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H2(g) ⇌ H2O(g) + Cu(s) Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

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Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g) ⇌\rightleftharpoons⇌ CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

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At 250ºC, the equilibrium constant Kp for the reaction PCl5(g) ⇌\rightleftharpoons⇌ PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium.

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For the reaction H2(g) + I2(g) ⇌ 2HI(g), KP = Kc.

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75.0 g of PCl5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) , and the system is allowed to reach equilibrium at 250ºC.PCl5(g) ⇌ PCl3(g) + Cl2(g) If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium

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For the reaction at equilibrium 2SO3 ⇌ 2SO2 + O2 ( Δ\DeltaΔ Hºrxn= 198 kJ/mol) , increasing the reaction temperature would:

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The equilibrium constant for the reaction Ni(s) + 4CO(g) ⇌\rightleftharpoons⇌ Ni(CO) 4(g) is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO) 4(g) ⇌\rightleftharpoons⇌ Ni(s) + 4CO(g)

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For the nitrogen fixation reaction 3H2(g) + N2(g) ⇌ 2NH3(g) , Kc = 6.0 * 10-2 at 500 ∘\circ∘ C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2

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Hydrogen iodide decomposes according to the equation 2HI(g) ⇌\rightleftharpoons⇌ H2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

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1.25 moles of NOCl were placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, K_c, for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) .

Correct Answer
verified

Consider this reaction at equilibrium: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) , $\Delta$ Hº_rxn = -198 kJ/mol If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium

Correct Answer
verified

Correct Answer
verified

K_p for the reaction 4CuO(s) $\rightleftharpoons$ 2Cu₂O(s) + O₂(g) is 0.49 at 1024^$\circ$C. Calculate K_c at this temperature

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

Correct Answer
verified

Hydrogen iodide decomposes according to the equation: 2HI(g) ⇌ H₂(g) + I₂(g) , K_c = 0.0156 at 400ºC a 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.Calculate the concentration of HI at equilibrium.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is removed from the system at equilibrium, the hydrogen (H₂) concentration will increase.

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). The production of ammonia is an exothermic reaction. When heat is added to the equilibrium system it will shift to increase the amount of ammonia produced.

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction Fe₂O₃ (s) + 3H₂ (g) $\rightleftharpoons$ 2Fe (s) + 3H₂O (g)

Correct Answer
verified

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) ⇌ H₂O(g) + Cu(s) $\Delta$ Hº_rxn = -2.0 kJ/mol

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) $\rightleftharpoons$ CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

Correct Answer
verified

At 250ºC, the equilibrium constant K_p for the reaction PCl₅(g) $\rightleftharpoons$ PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
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For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), K_P = K_c.

Correct Answer
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75.0 g of PCl₅(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl₂(g) , and the system is allowed to reach equilibrium at 250ºC.PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) If K_p = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium

Correct Answer
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For the reaction at equilibrium 2SO₃ ⇌ 2SO₂ + O₂ ( $\Delta$ Hº_rxn= 198 kJ/mol) , increasing the reaction temperature would:

Correct Answer
verified

The equilibrium constant for the reaction Ni(s) + 4CO(g) $\rightleftharpoons$ Ni(CO) ₄(g) is 5.0 * 10⁴ at 25ºC. What is the equilibrium constant for the reaction Ni(CO) ₄(g) $\rightleftharpoons$ Ni(s) + 4CO(g)

Correct Answer
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For the nitrogen fixation reaction 3H₂(g) + N₂(g) ⇌ 2NH₃(g) , K_c = 6.0 * 10^-2 at 500^$\circ$C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Correct Answer
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