Consider the following equilibria: 2SO3(g) NEWLINE 2SO2(g)+ O2(g)Kc = 2.3 * 10-7 2NO3(g) 2NO2(g)+ O2(g)Kc = 1.4 * 10-3 Calculate the equilibrium constant for the reaction SO2(g)+ NO3(g) SO3(g)+ NO2(g)

A) 78 B) 1.3 * 10-2 C) 1.6 * 10-4 D) 3.2 * 10-10 E) 6.1 * 103 A) 78 B) 1.3 * 10-2 C) 1.6 * 10-4 D) 3.2 * 10-10 E) 6.1 * 103

The equilibrium constant expression for the reaction 2BrF5(g) Br2(g)+ 5F2(g)is

A) Kc = [Br2] [F2] / [BrF5] B) Kc = [Br2] [F2]5 / [BrF5]2 C) Kc = [Br2] [F2]2 / [BrF5]5 D) Kc = [BrF5]2 / [Br2][F2]5 E) Kc = 2[BrF5]2 / ([Br2] * 5[F2]5) A) Kc = [Br2] [F2] / [BrF5] B) Kc = [Br2] [F2]5 / [BrF5]2 C) Kc = [Br2] [F2]2 / [BrF5]5 D) Kc = [BrF5]2 / [Br2][F2]5 E) Kc = 2[BrF5]2 / ([Br2] * 5[F2]5)

When the reaction 2H2S(g) 2H2(g)+ S2(g)is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g)?

A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm

Which of these situations will result if some CH4(g)is removed from the reaction CO(g)+ 3H2(g) CH4(g)+ H2O(g)at equilibrium?

A) H2O will be consumed. B) More CH4 and H2O will be produced. C) Kp will decrease. D) More CO will be produced. E) No change will occur. A) H2O will be consumed. B) More CH4 and H2O will be produced. C) Kp will decrease. D) More CO will be produced. E) No change will occur.

Exam 14: Chemical Equilibrium

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 21

Consider the following equilibria: 2SO₃(g) _NEW_LINE 2SO₂(g)+ O₂(g)K_c = 2.3 * 10^-7 2NO₃(g) 2NO₂(g)+ O₂(g)K_c = 1.4 * 10^-3 Calculate the equilibrium constant for the reaction SO₂(g)+ NO₃(g) SO₃(g)+ NO₂(g)

(Multiple Choice)

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Question 22

The equilibrium constant expression for the reaction 2BrF₅(g) Br₂(g)+ 5F₂(g)is

(Multiple Choice)

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Question 23

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Calculate K_c.

(Short Answer)

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Question 24

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

(Multiple Choice)

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Question 25

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 Cu²⁺(aq)at equilibrium?

(Short Answer)

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Question 26

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added, a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

(True/False)

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Question 27

When the reaction 2H₂S(g) 2H₂(g)+ S₂(g)is carried out at 1065°C, K_p = 0.012. Starting with pure H₂S at 1065°, what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?

(Multiple Choice)

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Question 28

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 29

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.

(Short Answer)

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Question 30

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

(True/False)

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Question 31

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 32

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?

(Essay)

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Question 33

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 34

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If hydrogen gas is added to this system at equilibrium, which direction will the reaction shift?

(Short Answer)

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Question 35

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 these statements is true?

(Multiple Choice)

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Question 36

Which of these situations will result if some CH₄(g)is removed from the reaction CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)at equilibrium?

(Multiple Choice)

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Question 37

Hydrogen iodide decomposes according to the equation 2HI(g) 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.

(Multiple Choice)

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Question 38

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?

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Question 39

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

(Essay)

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Question 40

Showing 21 - 40 of 100

Exam 14: Chemical Equilibrium

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).

Consider the following equilibria: 2SO3(g) NEWLINE 2SO2(g)+ O2(g)Kc = 2.3 * 10-7 2NO3(g) 2NO2(g)+ O2(g)Kc = 1.4 * 10-3 Calculate the equilibrium constant for the reaction SO2(g)+ NO3(g) SO3(g)+ NO2(g)

The equilibrium constant expression for the reaction 2BrF5(g) Br2(g)+ 5F2(g)is

The data below refer to the following reaction: 2NO(g)+ Br2(g) 2NOBr(g) Calculate Kc.

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

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 Cu2+(aq)at equilibrium?

If the system 3H2(g)+ N2(g) 2NH3(g)is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.

When the reaction 2H2S(g) 2H2(g)+ S2(g)is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(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?

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.

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

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.

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?

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 the reaction N2(g)+ 3H2(g) 2NH3(g). If hydrogen gas is added to this system at equilibrium, which direction will the reaction shift?

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 these statements is true?

Which of these situations will result if some CH4(g)is removed from the reaction CO(g)+ 3H2(g) CH4(g)+ H2O(g)at equilibrium?

Hydrogen iodide decomposes according to the equation 2HI(g) 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.

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?

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10-18.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

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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 K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present.Estimate the equilibrium concentration of H₂(g).

Consider the following equilibria: 2SO₃(g) _NEW_LINE 2SO₂(g)+ O₂(g)K_c = 2.3 * 10^-7 2NO₃(g) 2NO₂(g)+ O₂(g)K_c = 1.4 * 10^-3 Calculate the equilibrium constant for the reaction SO₂(g)+ NO₃(g) SO₃(g)+ NO₂(g)

The equilibrium constant expression for the reaction 2BrF₅(g) Br₂(g)+ 5F₂(g)is

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Calculate K_c.

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

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 Cu²⁺(aq)at equilibrium?

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added, a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

When the reaction 2H₂S(g) 2H₂(g)+ S₂(g)is carried out at 1065°C, K_p = 0.012. Starting with pure H₂S at 1065°, what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?

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.

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

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.

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?

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.

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If hydrogen gas is added to this system at equilibrium, which direction will the reaction shift?

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 these statements is true?

Which of these situations will result if some CH₄(g)is removed from the reaction CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)at equilibrium?

Hydrogen iodide decomposes according to the equation 2HI(g) 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.

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?

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?