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

Consider the reactions of cadmium with the thiosulfate anion. Cd2+(aq) + S2O32-(aq) Cd(S2O3)(aq) K1 = 8.3 × 103 Cd(S2O3)(aq) + S2O32-(aq) Cd(S2O3)22-(aq) K2 = 2.5 × 102 What is the value for the equilibrium constant for the following reaction? Cd2+(aq) + 2S2O32-(aq) Cd(S2O3)22-(aq)

A) 0.030 B) 33 C) 8.1 × 103 D) 8.6 × 103 E) 2.1 × 106 A) 0.030 B) 33 C) 8.1 × 103 D) 8.6 × 103 E) 2.1 × 106

What is the mass-action expression, Qc , for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(l) + Cl2(g)

A) B) C) D) E) None of the above expressions is correct. A) B) C) D) E) None of the above expressions is correct.

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) N2O(g) + NO2(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

A) The partial pressure of NO will increase. B) The partial pressure of NO will decrease. C) The partial pressure of NO2 will increase. D) The partial pressures of NO and N2O will increase. E) All three partial pressures will increase. A) The partial pressure of NO will increase. B) The partial pressure of NO will decrease. C) The partial pressure of NO2 will increase. D) The partial pressures of NO and N2O will increase. E) All three partial pressures will increase.

The equilibrium constant, Kc , for the decomposition of COBr2 COBr2(g) CO(g) + Br2(g) Is 0.190. What is Kc for the following reaction? 2CO(g) + 2Br2(g) 2COBr2(g)

A) 0.0361 B) 2.63 C) 5.62 D) 10.5 E) 27.7 A) 0.0361 B) 2.63 C) 5.62 D) 10.5 E) 27.7

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO3(s) MgO(s) + CO2(g) A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?

A) The partial pressure of carbon dioxide present at equilibrium will increase. B) The partial pressure of carbon dioxide present at equilibrium will decrease. C) The partial pressure of carbon dioxide at equilibrium will be unchanged. D) The equilibrium constant will have to decrease to compensate for the decrease in volume. E) More information is needed in order to make a valid judgment. A) The partial pressure of carbon dioxide present at equilibrium will increase. B) The partial pressure of carbon dioxide present at equilibrium will decrease. C) The partial pressure of carbon dioxide at equilibrium will be unchanged. D) The equilibrium constant will have to decrease to compensate for the decrease in volume. E) More information is needed in order to make a valid judgment.

Ethane can be formed by reacting acetylene with hydrogen. C2H2(g) + 2H2(g) C2H6(g) F1F1F1S1F1F1F10H°rxn = -311 kJ Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) none of the above, unless a catalyst is present A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) none of the above, unless a catalyst is present

Exam 17: Equilibrium: the Extent of Chemical Reactions

The equilibrium constant, K_p, for the reaction H₂(g) + I₂(g) 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

(Multiple Choice)

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Question 61

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

(True/False)

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Question 62

There is a direct correlation between the speed of a reaction and its equilibrium constant.

(True/False)

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Question 63

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

(Multiple Choice)

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Question 64

Write the expressions for K_c and K_p for the reaction PH₃BCl₃(s) PH₃(g) + BCl₃(g)

(Essay)

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Question 65

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?

(Multiple Choice)

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Question 66

H₂SO₃(aq) HSO₃^-(aq) + H⁺(aq) K_c = 1.4 × 10^-2 H₂SO₃(aq) SO₃^2-(aq) + 2H⁺(aq) K_c = 9.1 × 10^-10 Given the above equilibrium constant data at 25 °C, what is the value of K_c at this temperature for the reaction HSO₃^-(aq) SO₃^2-(aq) + H⁺(aq)?

(Multiple Choice)

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Question 67

Consider the reactions of cadmium with the thiosulfate anion. Cd²⁺(aq) + S₂O₃^2-(aq) Cd(S₂O₃)(aq) K₁= 8.3 × 10³ Cd(S₂O₃)(aq) + S₂O₃^2-(aq) Cd(S₂O₃)₂^2-(aq) K₂= 2.5 × 10² What is the value for the equilibrium constant for the following reaction? Cd²⁺(aq) + 2S₂O₃^2-(aq) Cd(S₂O₃)₂^2-(aq)

(Multiple Choice)

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Question 68

Write the mass-action expression, Q_c, for the following chemical reaction. Sn²⁺(aq) + O₂(g) + 3H₂O(l) SnO₂(s) + 2H₃O⁺(aq)

(Multiple Choice)

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Question 69

What is the mass-action expression, Q_c , for the following chemical reaction? 4H₃O⁺(aq) + 2Cl^-(aq) + MnO₂(s) Mn²⁺(aq) + 6H₂O(l) + Cl₂(g)

(Multiple Choice)

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Question 70

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) N₂O(g) + NO₂(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

(Multiple Choice)

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Question 71

The equilibrium constant, K_c, for the decomposition of COBr₂ COBr₂(g) CO(g) + Br₂(g) Is 0.190. What is K_c for the following reaction? 2CO(g) + 2Br₂(g) 2COBr₂(g)

(Multiple Choice)

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Question 72

An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant K_c = 1.6 × 10^-2 and the rate constant k_fwd = 8.0 × 10^-7s^-1 what is the value of k_rev?

(Multiple Choice)

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Question 73

For a solution equilibrium, a change in concentration of a reactant or product does not change K_c.

(True/False)

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Question 74

The reaction system CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?

(Multiple Choice)

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Question 75

Write the mass-action expression, Q_c, for the following chemical reaction. 2Cu²⁺(aq) + 4I^-(aq) 2CuI(s) + I₂(aq)

(Multiple Choice)

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Question 76

At 25°C, the equilibrium constant K_c for the reaction 2A(g) B(g) + C(g) Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?

(Multiple Choice)

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Question 77

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO₃(s) MgO(s) + CO₂(g) A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?

(Multiple Choice)

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Question 78

Ethane can be formed by reacting acetylene with hydrogen. C₂H₂(g) + 2H₂(g) C₂H₆(g) H°_rxn = -311 kJ Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

(Multiple Choice)

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Question 79

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_p = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 104

Exam 17: Equilibrium: the Extent of Chemical Reactions

The equilibrium constant, Kp , for the reaction H2(g) + I2(g) 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, Kc, will also be doubled.

There is a direct correlation between the speed of a reaction and its equilibrium constant.

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)

Write the expressions for Kc and Kp for the reaction PH3BCl3(s) PH3(g) + BCl3(g)

H2SO3(aq) HSO3-(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10 Given the above equilibrium constant data at 25 °C, what is the value of Kc at this temperature for the reaction HSO3-(aq) SO32-(aq) + H+(aq)?

Consider the reactions of cadmium with the thiosulfate anion. Cd2+(aq) + S2O32-(aq) Cd(S2O3)(aq) K1 = 8.3 × 103 Cd(S2O3)(aq) + S2O32-(aq) Cd(S2O3)22-(aq) K2 = 2.5 × 102 What is the value for the equilibrium constant for the following reaction? Cd2+(aq) + 2S2O32-(aq) Cd(S2O3)22-(aq)

Write the mass-action expression, Qc , for the following chemical reaction. Sn2+(aq) + O2(g) + 3H2O(l) SnO2(s) + 2H3O+(aq)

What is the mass-action expression, Qc , for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(l) + Cl2(g)

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) N2O(g) + NO2(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

The equilibrium constant, Kc , for the decomposition of COBr2 COBr2(g) CO(g) + Br2(g) Is 0.190. What is Kc for the following reaction? 2CO(g) + 2Br2(g) 2COBr2(g)

An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant Kc = 1.6 × 10-2 and the rate constant kfwd = 8.0 × 10-7 s-1 what is the value of krev?

For a solution equilibrium, a change in concentration of a reactant or product does not change Kc.

The reaction system CS2(g) + 4H2(g) CH4(g) + 2H2S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?

Write the mass-action expression, Qc , for the following chemical reaction. 2Cu2+(aq) + 4I-(aq) 2CuI(s) + I2(aq)

At 25°C, the equilibrium constant Kc for the reaction 2A(g) B(g) + C(g) Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO3(s) MgO(s) + CO2(g) A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?

Ethane can be formed by reacting acetylene with hydrogen. C2H2(g) + 2H2(g) C2H6(g) H°rxn = -311 kJ Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) NH3(g) + HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The 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: Bonding, Structure, and Reactivity

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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The equilibrium constant, K_p, for the reaction H₂(g) + I₂(g) 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

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

Write the expressions for K_c and K_p for the reaction PH₃BCl₃(s) PH₃(g) + BCl₃(g)

H₂SO₃(aq) HSO₃^-(aq) + H⁺(aq) K_c = 1.4 × 10^-2 H₂SO₃(aq) SO₃^2-(aq) + 2H⁺(aq) K_c = 9.1 × 10^-10 Given the above equilibrium constant data at 25 °C, what is the value of K_c at this temperature for the reaction HSO₃^-(aq) SO₃^2-(aq) + H⁺(aq)?

Write the mass-action expression, Q_c, for the following chemical reaction. Sn²⁺(aq) + O₂(g) + 3H₂O(l) SnO₂(s) + 2H₃O⁺(aq)

What is the mass-action expression, Q_c , for the following chemical reaction? 4H₃O⁺(aq) + 2Cl^-(aq) + MnO₂(s) Mn²⁺(aq) + 6H₂O(l) + Cl₂(g)

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) N₂O(g) + NO₂(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

The equilibrium constant, K_c, for the decomposition of COBr₂ COBr₂(g) CO(g) + Br₂(g) Is 0.190. What is K_c for the following reaction? 2CO(g) + 2Br₂(g) 2COBr₂(g)

An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant K_c = 1.6 × 10^-2 and the rate constant k_fwd = 8.0 × 10^-7s^-1 what is the value of k_rev?

For a solution equilibrium, a change in concentration of a reactant or product does not change K_c.

The reaction system CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?

Write the mass-action expression, Q_c, for the following chemical reaction. 2Cu²⁺(aq) + 4I^-(aq) 2CuI(s) + I₂(aq)

At 25°C, the equilibrium constant K_c for the reaction 2A(g) B(g) + C(g) Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO₃(s) MgO(s) + CO₂(g) A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?

Ethane can be formed by reacting acetylene with hydrogen. C₂H₂(g) + 2H₂(g) C₂H₆(g) H°_rxn = -311 kJ Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_p = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.