Which of the following rate laws is consistent with the following mechanism A2(g) + C(g) ⇌ AC(g) + A(g) fast equilibrium (Kc1) AC(g) + B2(g) $\rarr$ AB2(g) + C(g) slow

A) Rate = k[A2][C] B) Rate = k[AB2][C]/[AC][B2] C) Rate = kKc1[A2][C][B2]/[A] D) Rate = [A][AB2]/[A2][B2] E) Rate = kKc1[AC][A]/[A2][C] A) Rate = k[A2][C] B) Rate = k[AB2][C]/[AC][B2] C) Rate = kKc1[A2][C][B2]/[A] D) Rate = [A][AB2]/[A2][B2] E) Rate = kKc1[AC][A]/[A2][C] C

Calculate Kp for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl2(g) at 400$\circ$C if Kc at 400$\circ$C for this reaction is 2.1 * 10-2.

A) 2.1 * 10-2 B) 1.7 * 10-3 C) 0.70 D) 1.2 E) 3.8 * 10-4 A) 2.1 * 10-2 B) 1.7 * 10-3 C) 0.70 D) 1.2 E) 3.8 * 10-4

Consider the reaction, N2(g) + 3H2(g) ⇌ 2NH3(g). Kc = 4.2 at 600 K.What is the value of Kc for 4 NH3(g) ⇌ 2N2(g) + 6H2(g)

A) 0.053 B) 0.055 C) 0.057 D) 0.059 E) None of the above A) 0.053 B) 0.055 C) 0.057 D) 0.059 E) None of the above

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase 2NOBr(g) ⇌ 2NO(g) + Br2(g), $\Delta$Hºrxn= 30 kJ/mol

A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. E) Add a catalyst A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. E) Add a catalyst

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) $\begin{array}{lccc} \text { Concentration (M) } & [\mathrm{NO}] & \left[\mathrm{Br}_{2}\right] & {[\mathrm{NOBr}]} \\ \hline \text { Initial } & 2.5 & 5.0 & 1.0 \\ \text { Equilibrium } & 2.0 & - & - \end{array}$ Calculate Kc.

A) 0.080 B) 0.10 C) 0.12 D) 0.14 E) None of the above A) 0.080 B) 0.10 C) 0.12 D) 0.14 E) None of the above

Sodium carbonate, Na2CO3(s), can be prepared by heating sodium bicarbonate, NaHCO3(s) as shown below.2NaHCO3(s) (⇌) Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be

A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm

On analysis, an equilibrium mixture for the reaction 2H2S(g) $\rightleftharpoons$2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

A) 1.6 B) 3.2 C) 12.8 D) 0.64 E) 0.8 A) 1.6 B) 3.2 C) 12.8 D) 0.64 E) 0.8

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) $\begin{array}{lccc} \text { Concentration (M) } & [\mathrm{NO}] & \left[\mathrm{Br}_{2}\right] & {[\mathrm{NOBr}]} \\ \hline \text { Initial } & 2.5 & 5.0 & 1.0 \\ \text { Equilibrium } & 2.0 & - & - \end{array}$ Find the concentration of NOBr when the system reaches equilibrium.

A) 1.1 M B) 1.3 M C) 1.5 M D) 1.7 M E) None of the above A) 1.1 M B) 1.3 M C) 1.5 M D) 1.7 M E) None of the above

The reaction 2SO3(g) ⇌2SO2(g) + O2(g) is endothermic. If the temperature is increased,

A) more SO3 will be produced. B) Kc will decrease. C) no change will occur in Kc . D) Kc will increase. E) the pressure will decrease. A) more SO3 will be produced. B) Kc will decrease. C) no change will occur in Kc . D) Kc will increase. E) the pressure will decrease.

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 mass of the solid in the vessel once equilibrium is reached

A) 6.9 g of solid B) 7.1 g of solid C) 7.3 g of solid D) 7.5 g of solid E) None of the above A) 6.9 g of solid B) 7.1 g of solid C) 7.3 g of solid D) 7.5 g of solid E) None of the above

Exam 14: Chemical Equilibrium

Consider the equilibrium equation C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The reaction will shift towards products if the volume of the container is decreased.

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Question 1

Correct Answer:

Verified

False

Which of the following rate laws is consistent with the following mechanism A₂(g) + C(g) ⇌ AC(g) + A(g) fast equilibrium (K_c1) AC(g) + B₂(g) $\rarr$ AB₂(g) + C(g) slow

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Question 2

Correct Answer:

Verified

At 340 K, K_p = 69 for the reaction H₂(g) + I₂(g) (⇌) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

25.0 g of HI(g) is injected into a 4.00 L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400ºC, what will be the total pressure inside the reaction vessel? 2HI(g) ⇌ H₂(g) + I₂(g), K_c = 0.0156 at 400ºC

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Question 4

The brown gas NO₂ and the colorless gas N₂O₄ exist in equilibrium, 2NO₂ $\rightleftharpoons$ N₂O₄. In an experiment, 0.625 mole of N₂O₄ was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N₂O₄ at equilibrium was 0.0750 M. Calculate K_c for the reaction.

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Question 5

If the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g) is carried out at 1065^$\circ$C, K_p = 0.0120. Starting from pure H₂S introduced into an evacuated vessel at 1065^$\circ$C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H₂(g)

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Question 6

Calculate K_p for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) at 400^$\circ$C if K_c at 400^$\circ$C for this reaction is 2.1 * 10^-2.

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Question 7

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). K_c = 4.2 at 600 K.What is the value of K_c for 4 NH₃(g) ⇌ 2N₂(g) + 6H₂(g)

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Question 8

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

(Multiple Choice)

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Question 9

For the following reaction at equilibrium, which gives a change that will shift the position of equilibrium to favor formation of more products 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

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Question 10

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Calculate K_c.

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Question 11

Sodium carbonate, Na₂CO₃(s), can be prepared by heating sodium bicarbonate, NaHCO₃(s) as shown below.2NaHCO₃(s) (⇌) Na₂CO₃(s) + CO₂(g) + H₂O(g) K_p = 0.23 at 100ºC If a sample of NaHCO₃ is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be

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Question 12

On analysis, an equilibrium mixture for the reaction 2H₂S(g) $\rightleftharpoons$ 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

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Question 13

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Using a catalyst will cause the reaction to shift to the right.

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Question 14

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science, and is shown below.CO₂(aq) + H₂O(l) ⇌ H₂CO₃(aq) Based on the equilibrium constant reported for this reaction (K_c = 1.70 * 10^-3), there will be more carbon dioxide in solution than carbonic acid.

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Question 15

15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25^$\circ$C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if K_p = 0.108 at 25^$\circ$C for NH₄HS(s) ⇌ NH₃(g) + H₂S (g)

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Question 16

50.0 g of N₂O₄ is introduced into an evacuated 2.00 L vessel and allowed to come to equilibrium with its decomposition product, N₂O₄(g) ⇌ 2NO₂(g). For this reaction K_c = 0.133. Once the system has reached equilibrium, 5.00 g of NO₂ is injected into the vessel, and the system is allowed to equilibrate once again. Calculate the mass of NO₂ in the final equilibrium mixture.

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Question 17

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of NOBr when the system reaches equilibrium.

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Question 18

The reaction 2SO₃(g) ⇌2SO₂(g) + O₂(g) is endothermic. If the temperature is increased,

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Question 19

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide as shown below.CaCO₃(s) ⇌ CaO(s) + CO₂(g) The K_P 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 mass of the solid in the vessel once equilibrium is reached

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Question 20

Showing 1 - 20 of 119

Consider the equilibrium equation C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The reaction will shift towards products if the volume of the container is decreased.

Which of the following rate laws is consistent with the following mechanism A₂(g) + C(g) ⇌ AC(g) + A(g) fast equilibrium (K_c1) AC(g) + B₂(g) $\rarr$ AB₂(g) + C(g) slow

At 340 K, K_p = 69 for the reaction H₂(g) + I₂(g) (⇌) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium

25.0 g of HI(g) is injected into a 4.00 L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400ºC, what will be the total pressure inside the reaction vessel? 2HI(g) ⇌ H₂(g) + I₂(g), K_c = 0.0156 at 400ºC

If the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g) is carried out at 1065^$\circ$C, K_p = 0.0120. Starting from pure H₂S introduced into an evacuated vessel at 1065^$\circ$C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H₂(g)

Calculate K_p for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) at 400^$\circ$C if K_c at 400^$\circ$C for this reaction is 2.1 * 10^-2.

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). K_c = 4.2 at 600 K.What is the value of K_c for 4 NH₃(g) ⇌ 2N₂(g) + 6H₂(g)

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

For the following reaction at equilibrium, which gives a change that will shift the position of equilibrium to favor formation of more products 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Calculate K_c.

On analysis, an equilibrium mixture for the reaction 2H₂S(g) $\rightleftharpoons$ 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Using a catalyst will cause the reaction to shift to the right.

15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25^$\circ$C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if K_p = 0.108 at 25^$\circ$C for NH₄HS(s) ⇌ NH₃(g) + H₂S (g)

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of NOBr when the system reaches equilibrium.

The reaction 2SO₃(g) ⇌2SO₂(g) + O₂(g) is endothermic. If the temperature is increased,

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Exam 14: Chemical Equilibrium

Consider the equilibrium equation C(s) + H2O(g) ⇌ CO(g) + H2(g), Δ\DeltaΔ H = 2296 J. The reaction will shift towards products if the volume of the container is decreased.

Which of the following rate laws is consistent with the following mechanism A2(g) + C(g) ⇌ AC(g) + A(g) fast equilibrium (Kc1) AC(g) + B2(g) →\rarr→ AB2(g) + C(g) slow

At 340 K, Kp = 69 for the reaction H2(g) + I2(g) (⇌) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium

25.0 g of HI(g) is injected into a 4.00 L reaction vessel that contains 20.0 g of I2(g). When the system comes to equilibrium at 400ºC, what will be the total pressure inside the reaction vessel? 2HI(g) ⇌ H2(g) + I2(g), Kc = 0.0156 at 400ºC

If the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is carried out at 1065 ∘\circ∘ C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065 ∘\circ∘ C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)

Calculate Kp for the reaction 2NOCl(g) ⇌\rightleftharpoons⇌ 2NO(g) + Cl2(g) at 400 ∘\circ∘ C if Kc at 400 ∘\circ∘ C for this reaction is 2.1 * 10-2.

Consider the reaction, N2(g) + 3H2(g) ⇌ 2NH3(g). Kc = 4.2 at 600 K.What is the value of Kc for 4 NH3(g) ⇌ 2N2(g) + 6H2(g)

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase 2NOBr(g) ⇌ 2NO(g) + Br2(g), Δ\DeltaΔ Hºrxn= 30 kJ/mol

For the following reaction at equilibrium, which gives a change that will shift the position of equilibrium to favor formation of more products 2NOBr(g) ⇌ 2NO(g) + Br2(g), Δ\DeltaΔ Hºrxn = 30 kJ/mol

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Calculate Kc.

On analysis, an equilibrium mixture for the reaction 2H2S(g) ⇌\rightleftharpoons⇌ 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). Using a catalyst will cause the reaction to shift to the right.

15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25 ∘\circ∘ C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if Kp = 0.108 at 25 ∘\circ∘ C for NH4HS(s) ⇌ NH3(g) + H2S (g)

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of NOBr when the system reaches equilibrium.

The reaction 2SO3(g) ⇌2SO2(g) + O2(g) is endothermic. If the temperature is increased,

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

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Consider the equilibrium equation C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The reaction will shift towards products if the volume of the container is decreased.

Which of the following rate laws is consistent with the following mechanism A₂(g) + C(g) ⇌ AC(g) + A(g) fast equilibrium (K_c1) AC(g) + B₂(g) $\rarr$ AB₂(g) + C(g) slow

At 340 K, K_p = 69 for the reaction H₂(g) + I₂(g) (⇌) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium

25.0 g of HI(g) is injected into a 4.00 L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400ºC, what will be the total pressure inside the reaction vessel? 2HI(g) ⇌ H₂(g) + I₂(g), K_c = 0.0156 at 400ºC

If the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g) is carried out at 1065^$\circ$C, K_p = 0.0120. Starting from pure H₂S introduced into an evacuated vessel at 1065^$\circ$C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H₂(g)

Calculate K_p for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) at 400^$\circ$C if K_c at 400^$\circ$C for this reaction is 2.1 * 10^-2.

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). K_c = 4.2 at 600 K.What is the value of K_c for 4 NH₃(g) ⇌ 2N₂(g) + 6H₂(g)

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

For the following reaction at equilibrium, which gives a change that will shift the position of equilibrium to favor formation of more products 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Calculate K_c.

On analysis, an equilibrium mixture for the reaction 2H₂S(g) $\rightleftharpoons$ 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Using a catalyst will cause the reaction to shift to the right.

15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25^$\circ$C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if K_p = 0.108 at 25^$\circ$C for NH₄HS(s) ⇌ NH₃(g) + H₂S (g)

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of NOBr when the system reaches equilibrium.

The reaction 2SO₃(g) ⇌2SO₂(g) + O₂(g) is endothermic. If the temperature is increased,