Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of c?

A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63 A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

A) adding N2 gas to double the pressure B) adding more solid NaOH C) decreasing the volume of the container D) removing half of the solid NaHCO3 E) None of these choices are correct. A) adding N2 gas to double the pressure B) adding more solid NaOH C) decreasing the volume of the container D) removing half of the solid NaHCO3 E) None of these choices are correct.

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) ΔH°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) None of these choices are correct. A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) None of these choices are correct.

At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) 2HCN(g)

A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104 A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104

Exam 17: Equilibrium the Extent of Chemical Reactions

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are 0.016 mol L^-1, what is the value of _c?

(Multiple Choice)

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Question 61

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

(Multiple Choice)

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Question 62

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

(Multiple Choice)

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Question 63

Unless ΔH°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

(True/False)

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Question 64

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

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Question 65

A chemical reaction will reach equilibrium when the limiting reactant is used up.

(True/False)

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Question 66

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g)₂ Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

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Question 67

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H₂(g) CH₃OH(g) ΔH°_rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

(Multiple Choice)

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Question 68

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

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Question 69

The reaction quotient, _c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

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Question 70

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

(Multiple Choice)

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Question 71

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br₂(g) NOBr(g)

(Multiple Choice)

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Question 72

The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

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Question 73

At high temperatures, carbon reacts with O₂ to produce CO as follows: C(s) + O₂(g) 2CO(g). When 0.350 mol of O₂ and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, K_c, for this reaction?

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Question 74

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

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Question 75

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N₂(g) + O₂(g) 2NO(g) The equilibrium constant K_p for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

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Question 76

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃)₃COH(g) (CH₃)₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

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Question 77

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) ΔH°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

(Multiple Choice)

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Question 78

For some gas-phase reactions, K_p = K_c.

(True/False)

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Question 79

At 500°C the equilibrium constant, K_p, is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is Kp for the following reaction? H₂(g) + C₂N₂(g) 2HCN(g)

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Question 80

Showing 61 - 80 of 97

Exam 17: Equilibrium the Extent of Chemical Reactions

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of c?

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO2(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Unless ΔH°rxn = 0, a change in temperature will affect the value of the equilibrium constant Kc.

In water, the following equilibrium exists: H+(aq) + OH-(aq) H2O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

A chemical reaction will reach equilibrium when the limiting reactant is used up.

At a certain temperature the reaction CO2(g) + H2(g) CO(g) + H2O(g)2 Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) CH3OH(g) ΔH°rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)

The reaction quotient, c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br2(g) NOBr(g)

The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when

At high temperatures, carbon reacts with O2 to produce CO as follows: C(s) + O2(g) 2CO(g). When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) (CH3)2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) ΔH°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

For some gas-phase reactions, Kp = Kc.

At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) 2HCN(g)

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces Liquids, Solids, and Phase Changes

The Properties of Mixtures Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are 0.016 mol L^-1, what is the value of _c?

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Unless ΔH°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g)₂ Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H₂(g) CH₃OH(g) ΔH°_rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

The reaction quotient, _c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br₂(g) NOBr(g)

The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃)₃COH(g) (CH₃)₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) ΔH°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

For some gas-phase reactions, K_p = K_c.

At 500°C the equilibrium constant, K_p, is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is Kp for the following reaction? H₂(g) + C₂N₂(g) 2HCN(g)