Which of the following rate laws is consistent with the following mechanism? A(g)+ B(g) AB(g)fast equilibrium (Kc1) AB(g)+ C(g)$\rarr$ AC(g)+ B(g)slow

A) Rate = k[A][B] B) Rate = kKc1[A][B][C] C) Rate = k[AC][B]/[AB][C] D) Rate = [AB]/[A][B] E) Rate = Kc1[AC]/[A][C] A) Rate = k[A][B] B) Rate = kKc1[A][B][C] C) Rate = k[AC][B]/[AB][C] D) Rate = [AB]/[A][B] E) Rate = Kc1[AC]/[A][C] B

Kp for the reaction CO2(g)+ C(s) 2CO(g)is 1.47 at 727°C.Calculate Kc at this temperature

A) 1.47 B) 121 C) 0.0246 D) 0.0179 E) 87.7 A) 1.47 B) 121 C) 0.0246 D) 0.0179 E) 87.7

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)4(g)is 5.0 × 104 at 25ºC.What is the equilibrium constant for the reaction Ni(CO)4(g) Ni(s)+ 4CO(g)?

A) 2.0 × 10-5 B) 2.5 × 109 C) 5.0 × 104 D) 5.0 × 10-4 E) 2.0 × 10-3 A) 2.0 × 10-5 B) 2.5 × 109 C) 5.0 × 104 D) 5.0 × 10-4 E) 2.0 × 10-3

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

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

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. 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.

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

Exam 14: Chemical Equilibrium

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?

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Question 1

Correct Answer:

Verified

A solution was prepared such that the initial concentrations of Cu²⁺(aq)and CN^-(aq)were 0.0120 M and 0.0400 M, respectively.These ions react according to the following chemical equation What will be the concentration of CN^-(aq)at equilibrium?

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(Short Answer)

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Question 2

Correct Answer:

Verified

8.4 × 10^-7 M

Which of the following rate laws is consistent with the following mechanism? A(g)+ B(g) $Which of the following rate laws is consistent with the following mechanism? A(g)+ B(g) AB(g)fast equilibrium (Kc1) AB(g)+ C(g) \rarr AC(g)+ B(g)slow$ AB(g)fast equilibrium (K_c1) AB(g)+ C(g) $\rarr$ AC(g)+ B(g)slow

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

When the following reaction is at equilibrium, which of these relationships is always true? 2 O₃(g) 3 O₂(g)

(Multiple Choice)

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Question 4

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).

(True/False)

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Question 5

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

(Multiple Choice)

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Question 6

K_p for the reaction CO₂(g)+ C(s) 2CO(g)is 1.47 at 727°C.Calculate K_c at this temperature

(Multiple Choice)

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Question 7

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)₄(g)is 5.0 × 10⁴ at 25ºC.What is the equilibrium constant for the reaction Ni(CO)₄(g) Ni(s)+ 4CO(g)?

(Multiple Choice)

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Question 8

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?

(Multiple Choice)

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Question 9

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

(Short Answer)

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Question 10

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 11

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 H₂ equilibrium.

(Short Answer)

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Question 12

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

(Multiple Choice)

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Question 13

When the following reaction is at equilibrium, which of these relationships is always true? 2NOCl(g) 2NO(g)+ Cl₂(g)

(Multiple Choice)

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Question 14

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 15

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?

(Multiple Choice)

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Question 16

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

(Short Answer)

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Question 17

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

(Short Answer)

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Question 18

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

(Short Answer)

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Question 19

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).

(Short Answer)

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Question 20

Showing 1 - 20 of 109

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?

A solution was prepared such that the initial concentrations of Cu²⁺(aq)and CN^-(aq)were 0.0120 M and 0.0400 M, respectively.These ions react according to the following chemical equation What will be the concentration of CN^-(aq)at equilibrium?

When the following reaction is at equilibrium, which of these relationships is always true? 2 O₃(g) 3 O₂(g)

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).

K_p for the reaction CO₂(g)+ C(s) 2CO(g)is 1.47 at 727°C.Calculate K_c at this temperature

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)₄(g)is 5.0 × 10⁴ at 25ºC.What is the equilibrium constant for the reaction Ni(CO)₄(g) Ni(s)+ 4CO(g)?

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

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?

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 H₂ equilibrium.

When the following reaction is at equilibrium, which of these relationships is always true? 2NOCl(g) 2NO(g)+ Cl₂(g)

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?

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?

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

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).

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Exam 14: Chemical Equilibrium

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?

A solution was prepared such that the initial concentrations of Cu2+(aq)and CN-(aq)were 0.0120 M and 0.0400 M, respectively.These ions react according to the following chemical equation What will be the concentration of CN-(aq)at equilibrium?

Which of the following rate laws is consistent with the following mechanism? A(g)+ B(g) AB(g)fast equilibrium (Kc1) AB(g)+ C(g) →\rarr→ AC(g)+ B(g)slow

When the following reaction is at equilibrium, which of these relationships is always true? 2 O3(g) 3 O2(g)

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).

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?

Kp for the reaction CO2(g)+ C(s) 2CO(g)is 1.47 at 727°C.Calculate Kc at this temperature

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)4(g)is 5.0 × 104 at 25ºC.What is the equilibrium constant for the reaction Ni(CO)4(g) Ni(s)+ 4CO(g)?

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?

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

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?

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 H2 equilibrium.

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?

When the following reaction is at equilibrium, which of these relationships is always true? 2NOCl(g) 2NO(g)+ Cl2(g)

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?

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?

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

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Two moles of PCl5 are placed in a 5.0 L container.Dissociation takes place according to the equation PCl5(g) PCl3(g)+ Cl2(g).At equilibrium, 0.40 mol of Cl2 are present.Calculate the equilibrium constant (Kc)for this reaction under the conditions of this experiment.

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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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?

A solution was prepared such that the initial concentrations of Cu²⁺(aq)and CN^-(aq)were 0.0120 M and 0.0400 M, respectively.These ions react according to the following chemical equation What will be the concentration of CN^-(aq)at equilibrium?

When the following reaction is at equilibrium, which of these relationships is always true? 2 O₃(g) 3 O₂(g)

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).

K_p for the reaction CO₂(g)+ C(s) 2CO(g)is 1.47 at 727°C.Calculate K_c at this temperature

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)₄(g)is 5.0 × 10⁴ at 25ºC.What is the equilibrium constant for the reaction Ni(CO)₄(g) Ni(s)+ 4CO(g)?

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

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?

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 H₂ equilibrium.

When the following reaction is at equilibrium, which of these relationships is always true? 2NOCl(g) 2NO(g)+ Cl₂(g)

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?

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?

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

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).