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 reaction SO2(g) + NO2(g) $\rightleftharpoons$ SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium

A) 0.48 mol/L B) 0.11 mol/L C) 0.95 mol/L D) 2.22 mol/L E) 18 mol/L A) 0.48 mol/L B) 0.11 mol/L C) 0.95 mol/L D) 2.22 mol/L E) 18 mol/L

For the reaction H2(g) + I2(g) ⇌ 2HI(g), Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which of the following is true based on the above

A) Qc > Kc, the reaction proceeds from left to right to reach equilibrium B) Qc > Kc, the reaction proceeds from right to left to reach equilibrium C) Qc c, the reaction proceeds from left to right to reach equilibrium D) Qc c, the reaction proceeds from right to left to reach equilibrium E) Qc = Kc, the reaction is currently at equilibrium A) Qc > Kc, the reaction proceeds from left to right to reach equilibrium B) Qc > Kc, the reaction proceeds from right to left to reach equilibrium C) Qc c, the reaction proceeds from left to right to reach equilibrium D) Qc c, the reaction proceeds from right to left to reach equilibrium E) Qc = Kc, the reaction is currently at equilibrium

Consider the following reactions and their associated equilibrium constants: $\begin{array}{ll} \mathrm{A}+2 \mathrm{~B} \leftrightharpoons \mathrm{C} & \mathrm{~K}_{1} \\ \mathrm{C} \leftrightharpoons \mathrm{D}+\mathrm{E} & \mathrm{~K}_{2} \end{array}$ For the reaction A + 2B (⇌) D + E, having equilibrium constant Kc,

A) Kc = K1 + K2 B) Kc = K1/K2 C) Kc = K1 - K2 D) Kc = (K1)(K2) E) Kc = K2/K1 A) Kc = K1 + K2 B) Kc = K1/K2 C) Kc = K1 - K2 D) Kc = (K1)(K2) E) Kc = K2/K1

At 700 K, the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Which of the following is true based on the above

A) Qc > Kc, the reaction proceeds from left to right to reach equilibrium B) Qc > Kc, the reaction proceeds from right to left to reach equilibrium C) Qc c, the reaction proceeds from left to right to reach equilibrium D) Qc c, the reaction proceeds from right to left to reach equilibrium E) Qc = Kc, the reaction is currently at equilibrium A) Qc > Kc, the reaction proceeds from left to right to reach equilibrium B) Qc > Kc, the reaction proceeds from right to left to reach equilibrium C) Qc c, the reaction proceeds from left to right to reach equilibrium D) Qc c, the reaction proceeds from right to left to reach equilibrium E) Qc = Kc, the reaction is currently at equilibrium

For the reaction at equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g), increasing the volume of the container would:

A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) Cause no change A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) Cause no change

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) $\rightleftharpoons$ COCl2(g) + Cl2(g), Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g) $\rightleftharpoons$ 2COCl2(g) + 2Cl2(g).

A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10 A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10

Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g), increasing the volume of the container would:

A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) Cause no change A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) Cause no change

Exam 14: Chemical 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 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

(Multiple Choice)

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Question 61

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

(Multiple Choice)

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Question 62

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

(Multiple Choice)

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Question 63

What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H₂(g) + I₂(g)

(Multiple Choice)

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Question 64

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).

(Multiple Choice)

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Question 65

For the reaction SO₂(g) + NO₂(g) $\rightleftharpoons$ SO₃(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20. L container, what concentration of SO₃ will be present at equilibrium

(Multiple Choice)

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Question 66

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), K_c = 50.2 at 445ºC. If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which of the following is true based on the above

(Multiple Choice)

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Question 67

The common allotropes of carbon (graphite and diamond) equilibrate as follows: C(gr) ⇌ C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm³/mol and 3.42 cm³/mol; $\Delta$ H_f of diamond is 1.90 kJ/mol. This data suggests that the formation of diamond is favored at

(Multiple Choice)

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Question 68

Consider the reaction N₂(g) + O₂(g) $\rightleftharpoons$ 2NO(g), for which K_c = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

(Multiple Choice)

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Question 69

Consider the following reactions and their associated equilibrium constants: +2\leftrightharpoons \leftrightharpoons+ For the reaction A + 2B (⇌) D + E, having equilibrium constant K_c,

(Multiple Choice)

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Question 70

At 700 K, the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) has the equilibrium constant K_c = 4.3 * 10⁶ , and the following concentrations are present: [SO₂] = 0.10 M; [SO₃] = 10. M; [O₂] = 0.10 M. Which of the following is true based on the above

(Multiple Choice)

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Question 71

The 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.

(Multiple Choice)

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Question 72

For the reaction at equilibrium: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g), increasing the volume of the container would:

(Multiple Choice)

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Question 73

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl₄(g) + ¹/₂O₂(g) $\rightleftharpoons$ COCl₂(g) + Cl₂(g), K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g) + O₂(g) $\rightleftharpoons$ 2COCl₂(g) + 2Cl₂(g).

(Multiple Choice)

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Question 74

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

(Multiple Choice)

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Question 75

Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g), increasing the volume of the container would:

(Multiple Choice)

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Question 76

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 77

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

(True/False)

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Question 78

Calculate K_c for the reaction 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

(Multiple Choice)

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Question 79

Consider the following equilibrium: 4NH₃(g) + 3O₂(g) ⇌ 2N₂(g) + 6H₂O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.

(True/False)

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Question 80

Showing 61 - 80 of 119

Exam 14: Chemical 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 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

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

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br2(g), Δ\DeltaΔ Hºrxn = 30 kJ/mol

What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H2(g) + I2(g)

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).

For the reaction SO2(g) + NO2(g) ⇌\rightleftharpoons⇌ SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium

For the reaction H2(g) + I2(g) ⇌ 2HI(g), Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which of the following is true based on the above

Consider the reaction N2(g) + O2(g) ⇌\rightleftharpoons⇌ 2NO(g), for which Kc = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, determine the equilibrium concentration of NO.

Consider the following reactions and their associated equilibrium constants: +2\leftrightharpoons \leftrightharpoons+ For the reaction A + 2B (⇌) D + E, having equilibrium constant Kc,

At 700 K, the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Which of the following is true based on the above

The 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 at equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g), increasing the volume of the container would:

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) ⇌\rightleftharpoons⇌ COCl2(g) + Cl2(g), Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g) ⇌\rightleftharpoons⇌ 2COCl2(g) + 2Cl2(g).

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

Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g), increasing the volume of the container would:

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 the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

Calculate Kc for the reaction 2HI(g) ⇌\rightleftharpoons⇌ H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Consider the following equilibrium: 4NH3(g) + 3O2(g) ⇌ 2N2(g) + 6H2O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.

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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 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M

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

For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left 2NOBr(g) ⇌ 2NO(g) + Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

What is the correct equilibrium constant expression for this reaction 2HI(g) ⇌ H₂(g) + I₂(g)

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).

For the reaction SO₂(g) + NO₂(g) $\rightleftharpoons$ SO₃(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20. L container, what concentration of SO₃ will be present at equilibrium

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), K_c = 50.2 at 445ºC. If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which of the following is true based on the above

Consider the reaction N₂(g) + O₂(g) $\rightleftharpoons$ 2NO(g), for which K_c = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

Consider the following reactions and their associated equilibrium constants: +2\leftrightharpoons \leftrightharpoons+ For the reaction A + 2B (⇌) D + E, having equilibrium constant K_c,

At 700 K, the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) has the equilibrium constant K_c = 4.3 * 10⁶ , and the following concentrations are present: [SO₂] = 0.10 M; [SO₃] = 10. M; [O₂] = 0.10 M. Which of the following is true based on the above

The 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 at equilibrium: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g), increasing the volume of the container would:

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

Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g), increasing the volume of the container would:

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 the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When nitrogen is added to the system at equilibrium, the reaction will shift toward the products.

Calculate K_c for the reaction 2HI(g) $\rightleftharpoons$ H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Consider the following equilibrium: 4NH₃(g) + 3O₂(g) ⇌ 2N₂(g) + 6H₂O(g) + 1531 kJ The concentrations of the products will increase when the temperature is increased.