The solubility of silver chloride can be increased by dissolving it in a solution containing ammonia.AgCl (s) $\rightleftharpoons$ Ag+ (aq) + Cl- (aq) K1 = 1.6 x 10-10 Ag+ (aq) + 2NH3 (aq) $\rightleftharpoons$ Ag(NH3)2+ (aq) K2 = 1.5 x 107 What is the value of the equilibrium constant for the overall reaction AgCl (s) + 2NH3 (aq) $\rightleftharpoons$ Ag(NH3)2+ (aq) + Cl- (aq) Knet =

A) 1.5 x 107 B) 2.4 x 10-3 C) 3.1 x 10-3 D) 2.3 x 1014 E) 2.4 x 107 A) 1.5 x 107 B) 2.4 x 10-3 C) 3.1 x 10-3 D) 2.3 x 1014 E) 2.4 x 107

The equilibrium constant expression for the reaction 2BrF5 (g) $\rightleftharpoons$ 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)

For the reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g), removing some of the product, Fe3O4(s), 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

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] = 0.010 M; [SO3] = 10. M; [O2] = 0.010 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

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.

A) 0.020 B) 0.040 C) 0.060 D) 0.080 E) None of the above A) 0.020 B) 0.040 C) 0.060 D) 0.080 E) None of the above

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) $\begin{array}{lccc} \text { Concentration (M) } & [\mathrm{NO}] & \left[\mathrm{Br}_{2}\right] & {[\mathrm{NOBr}]} \\ \hline \text { Initial } & 2.5 & 5.0 & 1.0 \\ \text { Equilibrium } & 2.0 & - & - \end{array}$ Find the concentration of Br2 when the system reaches equilibrium.

A) 4.15 M B) 4.75 M C) 4.95 M D) 5.05 M E) None of the above A) 4.15 M B) 4.75 M C) 4.95 M D) 5.05 M E) None of the above

Given the following information: 2A(g) + B(g) $\rightleftharpoons$ A2B(g) Kp1 2A(g) + C2(g) $\rightleftharpoons$ 2AC(g) Kp2 3/2A2(g) + B(g) + C(g) $\rightleftharpoons$ AC(g) + A2B(g) Kp3 Which relationship represents the equilibrium constant for the reaction: 3A2(g) + 3B(g) + 2C(g) $\rightleftharpoons$ 3A2B(g) + C2(g) Knet = ?

A) Knet = Kp1 x Kp2 x Kp3 B) Knet = Kp1 x 2Kp3 / Kp2 C) Knet = Kp1 - Kp2 + 2 Kp3 D) Knet = Kp1 x Kp32/ Kp2 E) Knet = Kp1 x Kp2 x Kp32 A) Knet = Kp1 x Kp2 x Kp3 B) Knet = Kp1 x 2Kp3 / Kp2 C) Knet = Kp1 - Kp2 + 2 Kp3 D) Knet = Kp1 x Kp32/ Kp2 E) Knet = Kp1 x Kp2 x Kp32

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 and a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

A) Kc = 15.3 B) Kc = 17.3 C) Kc = 19.3 D) Kc = 21.3 E) None of the above A) Kc = 15.3 B) Kc = 17.3 C) Kc = 19.3 D) Kc = 21.3 E) None of the above

The equilibrium constants for the chemical reaction N2(g) + O2(g) ⇌ 2NO(g) are KP = 1.1 * 10-3 and 3.6 * 10-3 at 2,200 K and 2,500 K, respectively.Which one of these statements is true

A) The reaction is exothermic, $\Delta$Hº P is less than Kc by a factor of (RT). D) The total pressure at 2,200 K is the same as at 2,500 K. E) Higher total pressure shifts the equilibrium to the left. A) The reaction is exothermic, $\Delta$Hº P is less than Kc by a factor of (RT). D) The total pressure at 2,200 K is the same as at 2,500 K. E) Higher total pressure shifts the equilibrium to the left.

Kp for the reaction of SO2(g) with O2 to produce SO3(g) is 3 * 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g) $\rightleftharpoons$ 2SO3(g).)

A) 3 * 1024 B) 5 * 1021 C) 2 * 1020 D) 5 * 1022 E) 7 * 1025 A) 3 * 1024 B) 5 * 1021 C) 2 * 1020 D) 5 * 1022 E) 7 * 1025

Exam 14: Chemical Equilibrium

The solubility of silver chloride can be increased by dissolving it in a solution containing ammonia.AgCl (s) $\rightleftharpoons$ Ag⁺ (aq) + Cl^- (aq) K₁ = 1.6 x 10^-10 Ag⁺ (aq) + 2NH₃ (aq) $\rightleftharpoons$ Ag(NH₃)₂⁺ (aq) K₂ = 1.5 x 10⁷ What is the value of the equilibrium constant for the overall reaction AgCl (s) + 2NH₃ (aq) $\rightleftharpoons$ Ag(NH₃)₂⁺ (aq) + Cl^- (aq) K_net =

(Multiple Choice)

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Question 81

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When hydrogen gas is added to this system at equilibrium, the reaction will shift towards reactants.

(True/False)

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Question 82

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 N₂(g).

(Multiple Choice)

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Question 83

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

(Multiple Choice)

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Question 84

For the reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g), removing some of the product, Fe₃O₄(s), would:

(Multiple Choice)

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Question 85

K_p for the reaction CO₂(g) + C(s) $\rightleftharpoons$ 2CO(g) is 1.47 at 727^$\circ$C. Calculate K_c at this temperature.

(Multiple Choice)

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Question 86

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] = 0.010 M; [SO₃] = 10. M; [O₂] = 0.010 M. Which of the following is true based on the above

(Multiple Choice)

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Question 87

50.0 g of N₂O₄ is introduced into an evacuated 2.00 L vessel and allowed to come to equilibrium with its decomposition product, N₂O₄(g) ⇌ 2NO₂(g). For this reaction K_c = 0.133. Once the system has reached equilibrium, 5.00 g of NO₂ is injected into the vessel, and the system is allowed to equilibrate once again. Calculate the mass of N₂O₄ in the final equilibrium mixture.

(Multiple Choice)

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Question 88

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.

(Multiple Choice)

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Question 89

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of Br₂ when the system reaches equilibrium.

(Multiple Choice)

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Question 90

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

(Multiple Choice)

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Question 91

Given the following information: 2A(g) + B(g) $\rightleftharpoons$ A₂B(g) K_p1 2A(g) + C₂(g) $\rightleftharpoons$ 2AC(g) K_p2 3/2A₂(g) + B(g) + C(g) $\rightleftharpoons$ AC(g) + A₂B(g) K_p3 Which relationship represents the equilibrium constant for the reaction: 3A₂(g) + 3B(g) + 2C(g) $\rightleftharpoons$ 3A₂B(g) + C₂(g) K_net = ?

(Multiple Choice)

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Question 92

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: Cu²⁺(aq) + 4CN^-(aq) Kc= 1.0 x 10²⁵ ⇌ Cu(CN)₄^2-(aq) What will be the concentration of Cu²⁺(aq) at equilibrium

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Question 93

A quantity of liquid methanol, CH₃OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH₃OH(g) ⇌ CO(g) + 2 H₂(g), K_c= 6.90*10^-2.If the concentration of H₂ in the equilibrium mixture is 0.426M, what mass of methanol was initially introduced into the vessel

(Multiple Choice)

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Question 94

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 carbon dioxide 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 95

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 and a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

(Multiple Choice)

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Question 96

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 carbon monoxide 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 97

The equilibrium constants for the chemical reaction N₂(g) + O₂(g) ⇌ 2NO(g) are K_P = 1.1 * 10^-3 and 3.6 * 10^-3 at 2,200 K and 2,500 K, respectively.Which one of these statements is true

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Question 98

K_p for the reaction of SO₂(g) with O₂ to produce SO₃(g) is 3 * 10²⁴ . Calculate K_c for this equilibrium at 25ºC. (The relevant reaction is 2SO₂(g) + O₂(g) $\rightleftharpoons$ 2SO₃(g).)

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Question 99

Equilibrium is established for the reaction 2X(s) + Y(g) $\rightleftharpoons$ 2Z(g) at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

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Question 100

Showing 81 - 100 of 119

Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When hydrogen gas is added to this system at equilibrium, the reaction will shift towards reactants.

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 N₂(g).

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

For the reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g), removing some of the product, Fe₃O₄(s), would:

K_p for the reaction CO₂(g) + C(s) $\rightleftharpoons$ 2CO(g) is 1.47 at 727^$\circ$C. Calculate K_c at this temperature.

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] = 0.010 M; [SO₃] = 10. M; [O₂] = 0.010 M. Which of the following is true based on the above

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.

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of Br₂ when the system reaches equilibrium.

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

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 and a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

The equilibrium constants for the chemical reaction N₂(g) + O₂(g) ⇌ 2NO(g) are K_P = 1.1 * 10^-3 and 3.6 * 10^-3 at 2,200 K and 2,500 K, respectively.Which one of these statements is true

K_p for the reaction of SO₂(g) with O₂ to produce SO₃(g) is 3 * 10²⁴ . Calculate K_c for this equilibrium at 25ºC. (The relevant reaction is 2SO₂(g) + O₂(g) $\rightleftharpoons$ 2SO₃(g).)

Equilibrium is established for the reaction 2X(s) + Y(g) $\rightleftharpoons$ 2Z(g) at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

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Exam 14: Chemical Equilibrium

Consider the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). When hydrogen gas is added to this system at equilibrium, the reaction will shift towards reactants.

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 N2(g).

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

For the reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g), removing some of the product, Fe3O4(s), would:

Kp for the reaction CO2(g) + C(s) ⇌\rightleftharpoons⇌ 2CO(g) is 1.47 at 727 ∘\circ∘ C. Calculate Kc at this temperature.

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] = 0.010 M; [SO3] = 10. M; [O2] = 0.010 M. Which of the following is true based on the above

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.

The data below refer to the following reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of Br2 when the system reaches equilibrium.

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

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 carbon dioxide 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.

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 and a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

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 carbon monoxide 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.

The equilibrium constants for the chemical reaction N2(g) + O2(g) ⇌ 2NO(g) are KP = 1.1 * 10-3 and 3.6 * 10-3 at 2,200 K and 2,500 K, respectively.Which one of these statements is true

Kp for the reaction of SO2(g) with O2 to produce SO3(g) is 3 * 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g) ⇌\rightleftharpoons⇌ 2SO3(g).)

Equilibrium is established for the reaction 2X(s) + Y(g) ⇌\rightleftharpoons⇌ 2Z(g) at 500K, Kc = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

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Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g). When hydrogen gas is added to this system at equilibrium, the reaction will shift towards reactants.

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 N₂(g).

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

For the reaction at equilibrium: 3Fe(s) + 4H₂O(g) ⇌ Fe₃O₄(s) + 4H₂(g), removing some of the product, Fe₃O₄(s), would:

K_p for the reaction CO₂(g) + C(s) $\rightleftharpoons$ 2CO(g) is 1.47 at 727^$\circ$C. Calculate K_c at this temperature.

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] = 0.010 M; [SO₃] = 10. M; [O₂] = 0.010 M. Which of the following is true based on the above

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.

The data below refer to the following reaction: 2NO(g) + Br₂(g) ⇌ 2NOBr(g) Concentration (M) [] [] Initial 2.5 5.0 1.0 Equilibrium 2.0 - - Find the concentration of Br₂ when the system reaches equilibrium.

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

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 and a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

The equilibrium constants for the chemical reaction N₂(g) + O₂(g) ⇌ 2NO(g) are K_P = 1.1 * 10^-3 and 3.6 * 10^-3 at 2,200 K and 2,500 K, respectively.Which one of these statements is true

K_p for the reaction of SO₂(g) with O₂ to produce SO₃(g) is 3 * 10²⁴ . Calculate K_c for this equilibrium at 25ºC. (The relevant reaction is 2SO₂(g) + O₂(g) $\rightleftharpoons$ 2SO₃(g).)

Equilibrium is established for the reaction 2X(s) + Y(g) $\rightleftharpoons$ 2Z(g) at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.