Consider the following equilibria: 2SO3(g) ⇌ 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

4.21 moles of S2Cl4 are introduced into a 2.0 L vessel.S2Cl4(g) ⇌ 2SCl2(g) At equilibrium, 1.25 moles of S2Cl4 are found to remain in the container. Calculate Kc for this reaction.

A) Kc = 10.0 B) Kc = 12.0 C) Kc = 14.0 D) Kc = 16.0 E) None of the above A) Kc = 10.0 B) Kc = 12.0 C) Kc = 14.0 D) Kc = 16.0 E) None of the above

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

Consider the two gaseous equilibria: $\begin{array}{ll} \mathrm{SO}_{2}(\mathrm{g})+~^1/_2 \mathrm{O}_{2}(\mathrm{~g}) \leftrightharpoons \mathrm{SO}_{3}(\mathrm{g}) & \mathrm{K}_{1} \\ 2 \mathrm{SO}_{3}(\mathrm{g}) \leftrightharpoons \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) & \mathrm{K}_{2} \end{array}$ The values of the equilibrium constants K1 and K2 are related by

A) K2 = K12 B) K22 = K1 C) K2 = 1/K12 D) K2 = 1/K1 E) none of these. A) K2 = K12 B) K22 = K1 C) K2 = 1/K12 D) K2 = 1/K1 E) none of these.

When the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is carried out at 1065$\circ$C, Kp = 0.012. Starting with pure H2S at 1065$\circ$, 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

A reaction with an equilibrium constant Kc = 1.5 x 1021 would consist of which of the following at equilibrium:

A) approximately equal reactants and products B) some reactants and products with reactants slightly favored C) some reactants and products with products slightly favored D) essentially all reactants E) essentially all products A) approximately equal reactants and products B) some reactants and products with reactants slightly favored C) some reactants and products with products slightly favored D) essentially all reactants E) essentially all products

Consider the reaction, N2(g) + 3H2(g) ⇌ 2NH3(g). Kc = 8.1 x 10-3 at 900 K.What is the value of Kc for NH3(g) ⇌ (1/2)N2(g) + 3/2H2(g)

A) 17 B) 15 C) 13 D) 11 E) None of the above A) 17 B) 15 C) 13 D) 11 E) None of the above

Exam 14: Chemical Equilibrium

Consider the following equilibria: 2SO₃(g) ⇌ 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)

4.9/5

(71)

Question 21

4.21 moles of S₂Cl₄ are introduced into a 2.0 L vessel.S₂Cl₄(g) ⇌ 2SCl₂(g) At equilibrium, 1.25 moles of S₂Cl₄ are found to remain in the container. Calculate K_c for this reaction.

(Multiple Choice)

4.8/5

(77)

Question 22

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: $\mathrm{Cu}^{2+}(a q)+4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cd}(\mathrm{CN})_{4}^{2-}(a q)$ $\mathrm{K}_{\mathrm{c}}=1.0 \times 10^{25}$ What will be the concentration of CN^-(aq) at equilibrium

(Multiple Choice)

4.7/5

(78)

Question 23

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

(True/False)

4.9/5

(90)

Question 24

For the equilibrium reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), $\Delta$ Hº_rxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase

(Multiple Choice)

4.9/5

(89)

Question 25

Consider the equilibrium C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The concentration of carbon monoxide will increase if the temperature of this system is raised.

(True/False)

4.8/5

(90)

Question 26

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

(Multiple Choice)

4.9/5

(89)

Question 27

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture

(Multiple Choice)

4.8/5

(78)

Question 28

Consider the two gaseous equilibria: ()+()\leftrightharpoons() 2()\leftrightharpoons()+() The values of the equilibrium constants K₁ and K₂ are related by

(Multiple Choice)

4.8/5

(93)

Question 29

When the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g) is carried out at 1065^$\circ$C, K_p = 0.012. Starting with pure H₂S at 1065^$\circ$, 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)

4.9/5

(62)

Question 30

A reaction with an equilibrium constant K_c = 1.5 x 10²¹ would consist of which of the following at equilibrium:

(Multiple Choice)

4.8/5

(81)

Question 31

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

(Multiple Choice)

4.7/5

(82)

Question 32

Equilibrium constants are known for the following reactions: S(s) + ³/₂O₂(g) ⇌ SO₃(g) K_c = 9.2 * 10²³ SO₃(g) ⇌ SO₂(g) + ¹/₂O₂(g) K_c = 4.8 * 10^{- 4} Thus, for the reaction S(s) + O₂(g) ⇌ SO₂(g), K_c = 4.4 * 10²⁰.

(True/False)

4.9/5

(81)

Question 33

A reaction with an equilibrium constant K_c = 1.5 x 10^-25 would consist of which of the following at equilibrium:

(Multiple Choice)

4.8/5

(79)

Question 34

Consider the equilibrium C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The concentration of carbon will not change if gaseous water is added to the system.

(True/False)

4.7/5

(89)

Question 35

Given the following data for the reaction: A(g) + 2B(s) ⇌ AB₂(g) Temperature () 300 1.2\times1 600 12 900 2.2\times1 This data represents an endothermic reaction.

(True/False)

4.8/5

(91)

Question 36

Consider this reaction at equilibrium at a total pressure P₁: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

(Multiple Choice)

4.9/5

(72)

Question 37

4.2 mol of oxygen and 4.0 mol of NO are introduced to an evacuated 0.50 L reaction vessel. At a specific temperature, the equilibrium 2NO(g) + O₂(g) ⇌ 2NO₂(g) is reached when [NO] = 1.6 M. Calculate K_c for the reaction at this temperature.

(Multiple Choice)

4.9/5

(88)

Question 38

2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g).Calculate the equilibrium constant, K_c, for the reaction.

(Multiple Choice)

4.8/5

(68)

Question 39

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). K_c = 8.1 x 10^-3 at 900 K.What is the value of K_c for NH₃(g) ⇌ (1/2)N₂(g) + 3/2H₂(g)

(Multiple Choice)

4.8/5

(61)

Question 40

Showing 21 - 40 of 119

Exam 14: Chemical Equilibrium

Consider the following equilibria: 2SO3(g) ⇌ 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)

4.21 moles of S2Cl4 are introduced into a 2.0 L vessel.S2Cl4(g) ⇌ 2SCl2(g) At equilibrium, 1.25 moles of S2Cl4 are found to remain in the container. Calculate Kc for this reaction.

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

For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), Δ\DeltaΔ Hºrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase

Consider the equilibrium C(s) + H2O(g) ⇌ CO(g) + H2(g), Δ\DeltaΔ H = 2296 J. The concentration of carbon monoxide will increase if the temperature of this system is raised.

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

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture

Consider the two gaseous equilibria: ()+()\leftrightharpoons() 2()\leftrightharpoons()+() The values of the equilibrium constants K1 and K2 are related by

When the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is carried out at 1065 ∘\circ∘ C, Kp = 0.012. Starting with pure H2S at 1065 ∘\circ∘ , 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 reaction with an equilibrium constant Kc = 1.5 x 1021 would consist of which of the following at equilibrium:

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

Equilibrium constants are known for the following reactions: S(s) + 3/2O2(g) ⇌ SO3(g) Kc = 9.2 * 1023 SO3(g) ⇌ SO2(g) + 1/2O2(g) Kc = 4.8 * 10- 4 Thus, for the reaction S(s) + O2(g) ⇌ SO2(g), Kc = 4.4 * 1020.

A reaction with an equilibrium constant Kc = 1.5 x 10-25 would consist of which of the following at equilibrium:

Consider the equilibrium C(s) + H2O(g) ⇌ CO(g) + H2(g), Δ\DeltaΔ H = 2296 J. The concentration of carbon will not change if gaseous water is added to the system.

Given the following data for the reaction: A(g) + 2B(s) ⇌ AB2(g) Temperature () 300 1.2\times1 600 12 900 2.2\times1 This data represents an endothermic reaction.

Consider this reaction at equilibrium at a total pressure P1: 2SO2(g) + O2(g) ⇌ 2SO3(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

4.2 mol of oxygen and 4.0 mol of NO are introduced to an evacuated 0.50 L reaction vessel. At a specific temperature, the equilibrium 2NO(g) + O2(g) ⇌ 2NO2(g) is reached when [NO] = 1.6 M. Calculate Kc for the reaction at this temperature.

2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation 2NOCl(g) ⇌\rightleftharpoons⇌ 2NO(g) + Cl2(g).Calculate the equilibrium constant, Kc, for the reaction.

Consider the reaction, N2(g) + 3H2(g) ⇌ 2NH3(g). Kc = 8.1 x 10-3 at 900 K.What is the value of Kc for NH3(g) ⇌ (1/2)N2(g) + 3/2H2(g)

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Consider the following equilibria: 2SO₃(g) ⇌ 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)

4.21 moles of S₂Cl₄ are introduced into a 2.0 L vessel.S₂Cl₄(g) ⇌ 2SCl₂(g) At equilibrium, 1.25 moles of S₂Cl₄ are found to remain in the container. Calculate K_c for this reaction.

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

For the equilibrium reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), $\Delta$ Hº_rxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase

Consider the equilibrium C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The concentration of carbon monoxide will increase if the temperature of this system is raised.

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

Consider the two gaseous equilibria: ()+()\leftrightharpoons() 2()\leftrightharpoons()+() The values of the equilibrium constants K₁ and K₂ are related by

When the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g) is carried out at 1065^$\circ$C, K_p = 0.012. Starting with pure H₂S at 1065^$\circ$, 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 reaction with an equilibrium constant K_c = 1.5 x 10²¹ would consist of which of the following at equilibrium:

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

Equilibrium constants are known for the following reactions: S(s) + ³/₂O₂(g) ⇌ SO₃(g) K_c = 9.2 * 10²³ SO₃(g) ⇌ SO₂(g) + ¹/₂O₂(g) K_c = 4.8 * 10^{- 4} Thus, for the reaction S(s) + O₂(g) ⇌ SO₂(g), K_c = 4.4 * 10²⁰.

A reaction with an equilibrium constant K_c = 1.5 x 10^-25 would consist of which of the following at equilibrium:

Consider the equilibrium C(s) + H₂O(g) ⇌ CO(g) + H₂(g), $\Delta$ H = 2296 J. The concentration of carbon will not change if gaseous water is added to the system.

Given the following data for the reaction: A(g) + 2B(s) ⇌ AB₂(g) Temperature () 300 1.2\times1 600 12 900 2.2\times1 This data represents an endothermic reaction.

Consider this reaction at equilibrium at a total pressure P₁: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

4.2 mol of oxygen and 4.0 mol of NO are introduced to an evacuated 0.50 L reaction vessel. At a specific temperature, the equilibrium 2NO(g) + O₂(g) ⇌ 2NO₂(g) is reached when [NO] = 1.6 M. Calculate K_c for the reaction at this temperature.

2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g).Calculate the equilibrium constant, K_c, for the reaction.

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). K_c = 8.1 x 10^-3 at 900 K.What is the value of K_c for NH₃(g) ⇌ (1/2)N₂(g) + 3/2H₂(g)