Consider the following reaction: NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

A) 0.78 bar B) 0.084 bar C) 0.012 bar D) 0.85 bar E) 0.048 bar A) 0.78 bar B) 0.084 bar C) 0.012 bar D) 0.85 bar E) 0.048 bar

Calculate P (NO)eq, if P(NOCl)eq = 0.33 bar, P(Cl2)eq = 0.50 bar, and Kp = 1.9 × 10-2 bar . 2NOCl(g)⇌ 2NO(g)+ Cl2(g)

A) 1.7 bar B) 0.0042 bar C) 0.30 bar D) 0.064 bar E) 0.087 bar A) 1.7 bar B) 0.0042 bar C) 0.30 bar D) 0.064 bar E) 0.087 bar

The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g)+ O2(g)⇌ 2SO3(g) If initial concentrations are [SO2] = 6.00 mol L-1, [O2] = 0.45 mol L-1, and [SO3] = 9.00 mol L-1, the system is

A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state. A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state.

Consider the following reaction: CH4(g)+ 2H2S(g)⇌ CS2(g)+ 4H2(g) A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1)for the reaction.

A) 0.23 mol2 L-2 B) 0.038 mol2 L-2 C) 2.9 mol2 L-2 D) 10. mol2 L-2 E) 0.34 mol2 L-2 A) 0.23 mol2 L-2 B) 0.038 mol2 L-2 C) 2.9 mol2 L-2 D) 10. mol2 L-2 E) 0.34 mol2 L-2

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250° 0.125 mol L-1 PCl5 is added to the flask. If Kc = 1.80 mol L-1, what are the equilibrium concentrations of each gas?

A) [PCl5] = 0.00765 mol L-1, [PCl3] = 0.117 mol L-1, and [Cl2] = 0.117 mol L-1 B) [PCl5] = 0.0625 mol L-1, [PCl3] = 0.335 mol L-1, and [Cl2] = 0.335 mol L-1 C) [PCl5] = 1.80 mol L-1, [PCl3] = 1.80 mol L-1, and [Cl2] = 1.80 mol L-1 D) [PCl5] = 3.96 mol L-1, [PCl3] = 3.83 mol L-1, and [Cl2] = 3.83 mol L-1 A) [PCl5] = 0.00765 mol L-1, [PCl3] = 0.117 mol L-1, and [Cl2] = 0.117 mol L-1 B) [PCl5] = 0.0625 mol L-1, [PCl3] = 0.335 mol L-1, and [Cl2] = 0.335 mol L-1 C) [PCl5] = 1.80 mol L-1, [PCl3] = 1.80 mol L-1, and [Cl2] = 1.80 mol L-1 D) [PCl5] = 3.96 mol L-1, [PCl3] = 3.83 mol L-1, and [Cl2] = 3.83 mol L-1

Exam 14: Chemical Equilibrium

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl)_eq = 0.22 atm, P(NO)_eq = 0.10 atm, P(Cl₂)_eq = 0.081 atm. 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

(Multiple Choice)

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Question 21

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

(Multiple Choice)

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Question 22

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 0.039 mol L^-1

(Multiple Choice)

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Question 23

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g)⇌ 2NO₂(g)K = 1.46 2N₂O₄(g)⇌ 4NO₂(g)K = ?

(Multiple Choice)

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Question 24

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃. Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

(Multiple Choice)

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Question 25

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

(Multiple Choice)

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Question 26

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₃(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) K_c = 1.7 × 10⁸M^-1 [SO₂]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

(Multiple Choice)

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Question 27

Calculate P (NO)_eq, if P(NOCl)_eq = 0.33 bar, P(Cl₂)_eq = 0.50 bar, and K_p = 1.9 × 10^-2 bar . 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

(Multiple Choice)

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Question 28

The equilibrium constant is equal to 5.00 L mol^-1 at 1300 K for the reaction: 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) If initial concentrations are [SO₂] = 6.00 mol L^-1, [O₂] = 0.45 mol L^-1, and [SO₃] = 9.00 mol L^-1, the system is

(Multiple Choice)

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Question 29

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8M³ [NH₃]_eq = 2.9 × 10^-3 mol L^-1

(Multiple Choice)

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Question 30

Consider the following reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1)for the reaction.

(Multiple Choice)

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Question 31

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 mol L^-1 PCl₅ is added to the flask. If K_c = 1.80 mol L^-1, what are the equilibrium concentrations of each gas?

(Multiple Choice)

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Question 32

How is the reaction quotient different from an equilibrium constant for a given reaction?

(Essay)

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Question 33

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H₂. D₂(g)+ H₂(g)⇌ 2HD(g)K_p = 1.80 P(D₂)_eq = 1.1 × 10^-3bar P(HD)_eq = 2.7 × 10^-3 bar

(Multiple Choice)

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Question 34

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g)⇌ H₂(g)+ D₂(g) K = 0.28 2H₂(g)+ 2D₂(g)⇌ 4HD(g)K = ?

(Multiple Choice)

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Question 35

Can the K_p and K_c for a reaction ever have the same value? Why or why not?

(Essay)

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Question 36

Why aren't solids or liquids included in an equilibrium expression?

(Essay)

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Question 37

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

(Multiple Choice)

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Question 38

Match the following. -Q > K

(Multiple Choice)

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Question 39

For the following reaction, what is Δn required in the conversion of K_c to K_p? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

(Multiple Choice)

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Question 40

Showing 21 - 40 of 123

Exam 14: Chemical Equilibrium

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm, P(NO)eq = 0.10 atm, P(Cl2)eq = 0.081 atm. 2NOCl(g)⇌ 2NO(g)+ Cl2(g)

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO2(g)+ O2(g)⇌ 2SO3(g)

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g)⇌ 2NO2(g) Kc = 0.21 M [N2O4]eq = 0.039 mol L-1

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N2O4(g)⇌ 2NO2(g)K = 1.46 2N2O4(g)⇌ 4NO2(g)K = ?

Consider the following reaction: NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g). 2SO2(g)+ O2(g)⇌ 2SO3(g) Kc = 1.7 × 108 M-1 [SO2]eq = 0.0034 mol L-1 [O2]eq = 0.0018 mol L-1

Calculate P (NO)eq, if P(NOCl)eq = 0.33 bar, P(Cl2)eq = 0.50 bar, and Kp = 1.9 × 10-2 bar . 2NOCl(g)⇌ 2NO(g)+ Cl2(g)

The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g)+ O2(g)⇌ 2SO3(g) If initial concentrations are [SO2] = 6.00 mol L-1, [O2] = 0.45 mol L-1, and [SO3] = 9.00 mol L-1, the system is

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g). NH2COONH4(s)⇌ 2NH3(g)+ CO2(g)Kc = 1.58 × 10-8 M3 [NH3]eq = 2.9 × 10-3 mol L-1

Consider the following reaction: CH4(g)+ 2H2S(g)⇌ CS2(g)+ 4H2(g) A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S. If the equilibrium concentration of H2 is 0.44 mol L-1, find the equilibrium constant (mol L-1)for the reaction.

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250° 0.125 mol L-1 PCl5 is added to the flask. If Kc = 1.80 mol L-1, what are the equilibrium concentrations of each gas?

How is the reaction quotient different from an equilibrium constant for a given reaction?

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H2. D2(g)+ H2(g)⇌ 2HD(g)Kp = 1.80 P(D2)eq = 1.1 × 10-3 bar P(HD)eq = 2.7 × 10-3 bar

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g)⇌ H2(g)+ D2(g) K = 0.28 2H2(g)+ 2D2(g)⇌ 4HD(g)K = ?

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Why aren't solids or liquids included in an equilibrium expression?

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Match the following. -Q > K

For the following reaction, what is Δn required in the conversion of Kc to Kp? 2SO2(g)+ O2(g)⇌ 2SO3(g)

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Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl)_eq = 0.22 atm, P(NO)_eq = 0.10 atm, P(Cl₂)_eq = 0.081 atm. 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 0.039 mol L^-1

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g)⇌ 2NO₂(g)K = 1.46 2N₂O₄(g)⇌ 4NO₂(g)K = ?

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃. Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₃(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) K_c = 1.7 × 10⁸M^-1 [SO₂]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

Calculate P (NO)_eq, if P(NOCl)_eq = 0.33 bar, P(Cl₂)_eq = 0.50 bar, and K_p = 1.9 × 10^-2 bar . 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

The equilibrium constant is equal to 5.00 L mol^-1 at 1300 K for the reaction: 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) If initial concentrations are [SO₂] = 6.00 mol L^-1, [O₂] = 0.45 mol L^-1, and [SO₃] = 9.00 mol L^-1, the system is

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8M³ [NH₃]_eq = 2.9 × 10^-3 mol L^-1

Consider the following reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1)for the reaction.

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 mol L^-1 PCl₅ is added to the flask. If K_c = 1.80 mol L^-1, what are the equilibrium concentrations of each gas?

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H₂. D₂(g)+ H₂(g)⇌ 2HD(g)K_p = 1.80 P(D₂)_eq = 1.1 × 10^-3bar P(HD)_eq = 2.7 × 10^-3 bar

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g)⇌ H₂(g)+ D₂(g) K = 0.28 2H₂(g)+ 2D₂(g)⇌ 4HD(g)K = ?

Can the K_p and K_c for a reaction ever have the same value? Why or why not?

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

For the following reaction, what is Δn required in the conversion of K_c to K_p? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)