Phosgene, COCl2, a poisonous gas, decomposes as follows. COCl2(g) CO(g) + Cl2(g). At 900.ºC, Kc = 0.083. What is KP at this temperature? (R = 0.08206 L • atm/K • mol)

A) 0.125 B) 8.0 C) 6.1 D) 0.16 E) 0.083 A) 0.125 B) 8.0 C) 6.1 D) 0.16 E) 0.083

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl2(g). What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

A) 1.60 × 10-2 B) 2.10 × 10-7 C) 62.8 D) 4.90 × 106 E) 3.20 × 109 A) 1.60 × 10-2 B) 2.10 × 10-7 C) 62.8 D) 4.90 × 106 E) 3.20 × 109

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

A) 3.3 M B) 2.7 M C) 0.20 M D) 0.083 M E) 0.058 M A) 3.3 M B) 2.7 M C) 0.20 M D) 0.083 M E) 0.058 M

The reaction 2H2O2(g) 2H2O(g) + O2(g) is exothermic, ΔHºrxn = -210 kJ/mol. Which one of the following is correct?

A) KP at 800 K is smaller than KP at 1200 K. B) Temperature does not affect KP C) KP depends only on the pressure. D) KP at 1200 K is smaller than KP at 800 K. E) KP depends on total pressure as well as temperature. A) KP at 800 K is smaller than KP at 1200 K. B) Temperature does not affect KP C) KP depends only on the pressure. D) KP at 1200 K is smaller than KP at 800 K. E) KP depends on total pressure as well as temperature.

At 400ºC, Kc = 64 for the equilibrium H2(g) + I2(g) 2HI(g). If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

A) 0.15 M B) 1.2 M C) 2.4 M D) 4.8 M E) 5.8 M A) 0.15 M B) 1.2 M C) 2.4 M D) 4.8 M E) 5.8 M

At what temperature is KP = 4.00 for the reaction N2O4(g) 2NO2(g)? (R = 8.314 J/K • mol)

A) 197°C B) 56°C C) 36°C D) 79°C E) 476°C A) 197°C B) 56°C C) 36°C D) 79°C E) 476°C

Exam 15: Chemical Equilibrium

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH₃(g) 3H₂(g) + N₂(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

(Short Answer)

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Question 21

Phosgene, COCl₂, a poisonous gas, decomposes as follows. COCl₂(g) CO(g) + Cl₂(g). At 900.ºC, K_c = 0.083. What is K_P at this temperature? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 22

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g). What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 23

For the reaction 2X(g) + Y(g) 2Z(g), K_c = 1.00 ×10³ at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

(Multiple Choice)

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Question 24

During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?

(Multiple Choice)

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Question 25

For the equilibrium A₂(g) 2A(g), if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between K_c and time as equilibrium is established?

(Multiple Choice)

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Question 26

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

(Multiple Choice)

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Question 27

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N₂(g) + O₂(g) 2NO(g) The equilibrium constant K_P for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

(Multiple Choice)

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Question 28

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 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

(Multiple Choice)

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Question 29

For the nitrogen fixation reaction, 3H₂(g) + N₂(g) 2NH₃(g), K_c = 6.0 × 10^-2 at 500°C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂?

(Multiple Choice)

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Question 30

When a reaction reaches ________, the concentration of the reactants and products will no longer change.

(Short Answer)

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Question 31

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position, regardless of the physical state of the substance involved.

(True/False)

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Question 32

The reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) is exothermic, ΔHº_rxn=-210 kJ/mol. Which one of the following is correct?

(Multiple Choice)

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Question 33

Consider the reaction N₂(g) + 3H₂(g) 2NH₃(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

(Short Answer)

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Question 34

Consider the reaction N₂(g) + O₂(g) 2NO(g), for which K_c = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ what is the equilibrium concentration of NO?

(Multiple Choice)

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Question 35

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion).

(Multiple Choice)

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Question 36

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

(Multiple Choice)

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Question 37

At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g). If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

(Multiple Choice)

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Question 38

At what temperature is K_P = 4.00 for the reaction N₂O₄(g) 2NO₂(g)? (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 39

Which equation is correct?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 146

Exam 15: Chemical Equilibrium

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH3(g) 3H2(g) + N2(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

Phosgene, COCl2, a poisonous gas, decomposes as follows. COCl2(g) CO(g) + Cl2(g). At 900.ºC, Kc = 0.083. What is KP at this temperature? (R = 0.08206 L • atm/K • mol)

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl2(g). What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

For the reaction 2X(g) + Y(g) 2Z(g), Kc = 1.00 ×103 at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?

For the equilibrium A2(g) 2A(g), if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established?

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

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 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

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

When a reaction reaches ________, the concentration of the reactants and products will no longer change.

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position, regardless of the physical state of the substance involved.

The reaction 2H2O2(g) 2H2O(g) + O2(g) is exothermic, ΔHºrxn = -210 kJ/mol. Which one of the following is correct?

Consider the reaction N2(g) + 3H2(g) 2NH3(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Consider the reaction N2(g) + O2(g) 2NO(g), for which Kc = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 what is the equilibrium concentration of NO?

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion).

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2NH3(g)

At 400ºC, Kc = 64 for the equilibrium H2(g) + I2(g) 2HI(g). If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

At what temperature is KP = 4.00 for the reaction N2O4(g) 2NO2(g)? (R = 8.314 J/K • mol)

Which equation is correct?

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5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH₃(g) 3H₂(g) + N₂(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

Phosgene, COCl₂, a poisonous gas, decomposes as follows. COCl₂(g) CO(g) + Cl₂(g). At 900.ºC, K_c = 0.083. What is K_P at this temperature? (R = 0.08206 L • atm/K • mol)

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g). What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

For the reaction 2X(g) + Y(g) 2Z(g), K_c = 1.00 ×10³ at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

For the equilibrium A₂(g) 2A(g), if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between K_c and time as equilibrium is established?

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

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 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

For the nitrogen fixation reaction, 3H₂(g) + N₂(g) 2NH₃(g), K_c = 6.0 × 10^-2 at 500°C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂?

The reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) is exothermic, ΔHº_rxn=-210 kJ/mol. Which one of the following is correct?

Consider the reaction N₂(g) + 3H₂(g) 2NH₃(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Consider the reaction N₂(g) + O₂(g) 2NO(g), for which K_c = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ what is the equilibrium concentration of NO?

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g). If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

At what temperature is K_P = 4.00 for the reaction N₂O₄(g) 2NO₂(g)? (R = 8.314 J/K • mol)