Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g)ΔH° = -514 kJ Le Châtelier's principle predicts that removing O2 (g)to the reaction container will ________.

A) increase the partial pressure of CO B) decrease the partial pressure of CO C) increase the partial pressure of CO2 D) increase the value of the equilibrium constant E) decrease the value of the equilibrium constant A) increase the partial pressure of CO B) decrease the partial pressure of CO C) increase the partial pressure of CO2 D) increase the value of the equilibrium constant E) decrease the value of the equilibrium constant

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3 (g)+ Cl2 (g) → PCl5 (g) An equilibrium mixture at 450 K contains PPCl3 = 0.224 atm, PCl2 = 0.284 atm, and PPCl5 = 4.24 atm. What is the value of Kp at this temperature?

A) 66.7 B) 1.50 × 10-2 C) 2.70 × 10-1 D) 3.74 E) 8.36 A) 66.7 B) 1.50 × 10-2 C) 2.70 × 10-1 D) 3.74 E) 8.36

Consider the following reaction at equilibrium: C (s) + H2O (g) CO (g) + H2 (g) Which of the following conditions will decrease the partial pressure of CO?

A) decreasing the volume of the reaction vessel B) increasing the volume of the reaction vessel C) decreasing the amount of carbon in the system D) decreasing the pressure of the reaction vessel E) adding a catalyst to the reaction system A) decreasing the volume of the reaction vessel B) increasing the volume of the reaction vessel C) decreasing the amount of carbon in the system D) decreasing the pressure of the reaction vessel E) adding a catalyst to the reaction system

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

A) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm. C) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. D) The equilibrium partial pressure of BrCl (g)will be greater than 2.00 atm. E) The reaction will go to completion since there are equal amounts of Br2 and Cl2. A) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm. C) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. D) The equilibrium partial pressure of BrCl (g)will be greater than 2.00 atm. E) The reaction will go to completion since there are equal amounts of Br2 and Cl2.

The Kp for the reaction below is 1.49 × 108 at 100.0 °C: CO (g)+ Cl2 (g) → COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 1.00 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is ________ atm.

A) 1.49 B) 1.49 × 1016 C) 6.71 × 10-17 D) 1.49 × 104 E) 1.49 × 1012 A) 1.49 B) 1.49 × 1016 C) 6.71 × 10-17 D) 1.49 × 104 E) 1.49 × 1012

The equilibrium constant (Kp)for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5 giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is ________ atm.

A) 0.0782 B) 0.0455 C) 0.0908 D) 0.0330 E) 0.123 A) 0.0782 B) 0.0455 C) 0.0908 D) 0.0330 E) 0.123

Given the following reaction at equilibrium at 300.0 K: NH4HS (s) NH3 (g) + H2S (g) If pNH3 = pH2S = 0.105 atm, Kp = ________.

A) .0110 B) 4.99 × 10-4 C) .105 D) .0821 E) 5.66 × 10-3 A) .0110 B) 4.99 × 10-4 C) .105 D) .0821 E) 5.66 × 10-3

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.20 M, 0.034 M, and 0.55 M, respectively. The value of Keq for this reaction is ________.

A) 23 B) 81 C) 0.0090 D) 5.1 E) 44 A) 23 B) 81 C) 0.0090 D) 5.1 E) 44

The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g) + O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? NO2 (g) NO (g) + O2 (g)

A) 5.4 × 10-13 B) 5.4 × 1013 C) 1.4 × 10-7 D) 5.66 × 10-3 E) none of the above A) 5.4 × 10-13 B) 5.4 × 1013 C) 1.4 × 10-7 D) 5.66 × 10-3 E) none of the above

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g) → 2NO2 (g) A 1.000-L flask is charged with 9.20 × 10-3 mol of N2O4. At equilibrium, 5.98 × 10-3 mol of N2O4 remains. Keq for this reaction is ________.

A) 0.183 B) 0.197 C) 0.212 D) 6.94 × 10-3 E) 2.96 × 10-5 A) 0.183 B) 0.197 C) 0.212 D) 6.94 × 10-3 E) 2.96 × 10-5

Exam 15: Chemical Equilibrium

In which of the following reactions would increasing pressure at constant temperature change the concentrations of reactants and products, based on Le Châteliers principle?

(Multiple Choice)

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Question 81

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that removing O₂ (g)to the reaction container will ________.

(Multiple Choice)

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Question 82

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl₃ (g)+ Cl₂ (g) → PCl₅ (g) An equilibrium mixture at 450 K contains P_PCl₃ = 0.224 atm, P_Cl₂ = 0.284 atm, and P_PCl₅ = 4.24 atm. What is the value of K_p at this temperature?

(Multiple Choice)

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Question 83

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO₂ (g)+ 2H₂ (g) CH₃OH (g)

(Multiple Choice)

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Question 84

Consider the following reaction at equilibrium: C (s) + H₂O (g) CO (g) + H₂ (g) Which of the following conditions will decrease the partial pressure of CO?

(Multiple Choice)

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Question 85

At 400 K, the equilibrium constant for the reaction Br₂ (g) + Cl₂ (g) 2BrCl (g) Is K_p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g), 1.00 atm of Cl₂ (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

(Multiple Choice)

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Question 86

At 24° C, K_p = 0.080 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm)of ammonia, assuming that some solid NH₄HS remains.

(Multiple Choice)

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Question 87

The K_p for the reaction below is 1.49 × 10⁸ at 100.0 °C: CO (g)+ Cl₂ (g) → COCl₂ (g) In an equilibrium mixture of the three gases, P_CO = P_Cl₂ = 1.00 × 10^-4 atm. The partial pressure of the product, phosgene (COCl₂), is ________ atm.

(Multiple Choice)

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Question 88

The equilibrium constant (K_p)for the interconversion of PCl₅ and PCl₃ is 0.0121: PCl₅ (g) PCl₃ (g) + Cl₂ (g) A vessel is charged with PCl₅ giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is ________ atm.

(Multiple Choice)

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Question 89

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g) + H₂S (g) If pNH₃ = pH₂S = 0.105 atm, K_p = ________.

(Multiple Choice)

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Question 90

Consider the following chemical reaction: H₂ (g) + I₂ (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.20 M, 0.034 M, and 0.55 M, respectively. The value of K_eq for this reaction is ________.

(Multiple Choice)

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Question 91

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g) + O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? NO₂ (g) NO (g) + O₂ (g)

(Multiple Choice)

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Question 92

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N₂O₄ (g) → 2NO₂ (g) A 1.000-L flask is charged with 9.20 × 10^-3 mol of N₂O₄. At equilibrium, 5.98 × 10^-3 mol of N₂O₄ remains. K_eq for this reaction is ________.

(Multiple Choice)

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Question 93

The equilibrium-constant expression depends on the ________ of the reaction.

(Multiple Choice)

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Question 94

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

(Multiple Choice)

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Question 95

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N₂O₄ (g) 2NO₂ (g)

(Multiple Choice)

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Question 96

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq)+ H₂O (l) H₃O⁺ (aq)+ F^- (aq)

(Multiple Choice)

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Question 97

Showing 81 - 97 of 97

In which of the following reactions would increasing pressure at constant temperature change the concentrations of reactants and products, based on Le Châteliers principle?

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that removing O₂ (g)to the reaction container will ________.

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO₂ (g)+ 2H₂ (g) CH₃OH (g)

Consider the following reaction at equilibrium: C (s) + H₂O (g) CO (g) + H₂ (g) Which of the following conditions will decrease the partial pressure of CO?

At 400 K, the equilibrium constant for the reaction Br₂ (g) + Cl₂ (g) 2BrCl (g) Is K_p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g), 1.00 atm of Cl₂ (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

At 24° C, K_p = 0.080 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm)of ammonia, assuming that some solid NH₄HS remains.

The K_p for the reaction below is 1.49 × 10⁸ at 100.0 °C: CO (g)+ Cl₂ (g) → COCl₂ (g) In an equilibrium mixture of the three gases, P_CO = P_Cl₂ = 1.00 × 10^-4 atm. The partial pressure of the product, phosgene (COCl₂), is ________ atm.

The equilibrium constant (K_p)for the interconversion of PCl₅ and PCl₃ is 0.0121: PCl₅ (g) PCl₃ (g) + Cl₂ (g) A vessel is charged with PCl₅ giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is ________ atm.

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g) + H₂S (g) If pNH₃ = pH₂S = 0.105 atm, K_p = ________.

Consider the following chemical reaction: H₂ (g) + I₂ (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.20 M, 0.034 M, and 0.55 M, respectively. The value of K_eq for this reaction is ________.

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g) + O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? NO₂ (g) NO (g) + O₂ (g)

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N₂O₄ (g) → 2NO₂ (g) A 1.000-L flask is charged with 9.20 × 10^-3 mol of N₂O₄. At equilibrium, 5.98 × 10^-3 mol of N₂O₄ remains. K_eq for this reaction is ________.

The equilibrium-constant expression depends on the ________ of the reaction.

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N₂O₄ (g) 2NO₂ (g)

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq)+ H₂O (l) H₃O⁺ (aq)+ F^- (aq)

Introduction: Matter and Measurement

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Exam 15: Chemical Equilibrium

In which of the following reactions would increasing pressure at constant temperature change the concentrations of reactants and products, based on Le Châteliers principle?

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g)ΔH° = -514 kJ Le Châtelier's principle predicts that removing O2 (g)to the reaction container will ________.

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO2 (g)+ 2H2 (g) CH3OH (g)

Consider the following reaction at equilibrium: C (s) + H2O (g) CO (g) + H2 (g) Which of the following conditions will decrease the partial pressure of CO?

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

At 24° C, Kp = 0.080 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm)of ammonia, assuming that some solid NH4HS remains.

The Kp for the reaction below is 1.49 × 108 at 100.0 °C: CO (g)+ Cl2 (g) → COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 1.00 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is ________ atm.

The equilibrium constant (Kp)for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5 giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is ________ atm.

Given the following reaction at equilibrium at 300.0 K: NH4HS (s) NH3 (g) + H2S (g) If pNH3 = pH2S = 0.105 atm, Kp = ________.

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.20 M, 0.034 M, and 0.55 M, respectively. The value of Keq for this reaction is ________.

The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g) + O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? NO2 (g) NO (g) + O2 (g)

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g) → 2NO2 (g) A 1.000-L flask is charged with 9.20 × 10-3 mol of N2O4. At equilibrium, 5.98 × 10-3 mol of N2O4 remains. Keq for this reaction is ________.

The equilibrium-constant expression depends on the ________ of the reaction.

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g) 2NO2 (g)

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq)+ H2O (l) H3O+ (aq)+ F- (aq)

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that removing O₂ (g)to the reaction container will ________.

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO₂ (g)+ 2H₂ (g) CH₃OH (g)

Consider the following reaction at equilibrium: C (s) + H₂O (g) CO (g) + H₂ (g) Which of the following conditions will decrease the partial pressure of CO?

At 400 K, the equilibrium constant for the reaction Br₂ (g) + Cl₂ (g) 2BrCl (g) Is K_p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g), 1.00 atm of Cl₂ (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

At 24° C, K_p = 0.080 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm)of ammonia, assuming that some solid NH₄HS remains.

The K_p for the reaction below is 1.49 × 10⁸ at 100.0 °C: CO (g)+ Cl₂ (g) → COCl₂ (g) In an equilibrium mixture of the three gases, P_CO = P_Cl₂ = 1.00 × 10^-4 atm. The partial pressure of the product, phosgene (COCl₂), is ________ atm.

The equilibrium constant (K_p)for the interconversion of PCl₅ and PCl₃ is 0.0121: PCl₅ (g) PCl₃ (g) + Cl₂ (g) A vessel is charged with PCl₅ giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is ________ atm.

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g) + H₂S (g) If pNH₃ = pH₂S = 0.105 atm, K_p = ________.

Consider the following chemical reaction: H₂ (g) + I₂ (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.20 M, 0.034 M, and 0.55 M, respectively. The value of K_eq for this reaction is ________.

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g) + O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? NO₂ (g) NO (g) + O₂ (g)

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N₂O₄ (g) → 2NO₂ (g) A 1.000-L flask is charged with 9.20 × 10^-3 mol of N₂O₄. At equilibrium, 5.98 × 10^-3 mol of N₂O₄ remains. K_eq for this reaction is ________.

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N₂O₄ (g) 2NO₂ (g)

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq)+ H₂O (l) H₃O⁺ (aq)+ F^- (aq)