Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is sealed.If this solid decomposes according to the equation NH4HS(s) NH3(g)+ H2S(g), Kp = 0.108 at 25°C, What is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C?

A) 0.917 g B) 1.37 g C) 2.74 g D) 0.581 g E) 0.452 g A) 0.917 g B) 1.37 g C) 2.74 g D) 0.581 g E) 0.452 g

Sodium carbonate, Na2CO3(s), can be prepared by heating sodium bicarbonate, NaHCO3(s). 2NaHCO3(s) Na2CO3(s)+ CO2(g)+ H2O(g)Kp = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm

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] = 0.10 M; [SO3] = 10.M; [O2] = 0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium?

A) Yes, the mixture is at equilibrium. B) No, left to right C) No, right to left D) There is not enough information to be able to predict the direction. A) Yes, the mixture is at equilibrium. B) No, left to right C) No, right to left D) There is not enough information to be able to predict the direction.

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.

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. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium?

A) Yes, the mixture is at equilibrium. B) No, left to right C) No, right to left D) There is not enough information to be able to predict the direction. A) Yes, the mixture is at equilibrium. B) No, left to right C) No, right to left D) There is not enough information to be able to predict the direction.

Exam 14: Chemical Equilibrium

Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is sealed.If this solid decomposes according to the equation NH₄HS(s) NH₃(g)+ H₂S(g), K_p = 0.108 at 25°C, What is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C?

(Multiple Choice)

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Question 81

The brown gas NO₂ and the colorless gas N₂O₄ exist in equilibrium, 2NO₂ N₂O₄. In an experiment, 0.625 mole of N₂O₄ was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N₂O₄ at equilibrium was 0.0750 M. Calculate K_c for the reaction.

(Multiple Choice)

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Question 82

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq)+ H₂O(l) H₂CO₃(aq) Based on the equilibrium constant reported for this reaction (K_c = 1.70 * 10^-3), there will be more carbon dioxide in solution than carbonic acid.

(True/False)

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Question 83

Sodium carbonate, Na₂CO₃(s), can be prepared by heating sodium bicarbonate, NaHCO₃(s). 2NaHCO₃(s) Na₂CO₃(s)+ CO₂(g)+ H₂O(g)K_p = 0.23 at 100ºC If a sample of NaHCO₃ is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

(Multiple Choice)

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Question 84

For the reaction 2NOCl(g) 2NO(g)+ Cl₂(g), K_c = 8.0 at a certain temperature.What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

(Multiple Choice)

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Question 85

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion $\rarr$ greatest completion). $The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion \rarr greatest completion).$

(Multiple Choice)

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Question 86

Equilibrium is established for the reaction 2X(s)+ Y(g) 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.

(Multiple Choice)

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Question 87

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

(Short Answer)

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Question 88

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

(Short Answer)

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Question 89

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.

(Short Answer)

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Question 90

What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

(Essay)

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Question 91

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of Br₂ when the system reaches equilibrium.

(Short Answer)

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Question 92

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] = 0.10 M; [SO₃] = 10.M; [O₂] = 0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium?

(Multiple Choice)

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Question 93

Ethanol and acetic acid react to form ethyl acetate and water according to the following chemical equation: C₂H₅OH(l)+ CH₃COOH(l) CH₃COOC₂H₅(l)+ H₂O(l) When two moles each of ethanol and acetic acid are combined, equilibrium is reached when two-thirds of a mole of each of the reactants remains.Calculate the equilibrium constant for this reaction assuming total volume does not change during the course of the reaction.(Note: since water is not the solvent, but rather a product of the reaction, [H₂O] changes during the course of the reaction, so it should be included in the equilibrium constant expression.)

(Short Answer)

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Question 94

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).

(Short Answer)

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Question 95

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).What will happen to the mass of carbon if we add gaseous water to the system?

(Short Answer)

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Question 96

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 97

At 340 K, K_p = 69 for the reaction H₂(g)+ I₂(g) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium?

(Multiple Choice)

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Question 98

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?

(Multiple Choice)

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Question 99

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. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 100

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq)+ H₂O(l) H₂CO₃(aq) Based on the equilibrium constant reported for this reaction (K_c = 1.70 * 10^-3), there will be more carbon dioxide in solution than carbonic acid.

Sodium carbonate, Na₂CO₃(s), can be prepared by heating sodium bicarbonate, NaHCO₃(s). 2NaHCO₃(s) Na₂CO₃(s)+ CO₂(g)+ H₂O(g)K_p = 0.23 at 100ºC If a sample of NaHCO₃ is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

For the reaction 2NOCl(g) 2NO(g)+ Cl₂(g), K_c = 8.0 at a certain temperature.What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Equilibrium is established for the reaction 2X(s)+ Y(g) 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.

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

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.

What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of Br₂ when the system reaches equilibrium.

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).

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).What will happen to the mass of carbon if we add gaseous water to the system?

At 340 K, K_p = 69 for the reaction H₂(g)+ I₂(g) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium?

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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Exam 14: Chemical Equilibrium

The brown gas NO2 and the colorless gas N2O4 exist in equilibrium, 2NO2 N2O4. In an experiment, 0.625 mole of N2O4 was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction.

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2(aq)+ H2O(l) H2CO3(aq) Based on the equilibrium constant reported for this reaction (Kc = 1.70 * 10-3), there will be more carbon dioxide in solution than carbonic acid.

Sodium carbonate, Na2CO3(s), can be prepared by heating sodium bicarbonate, NaHCO3(s). 2NaHCO3(s) Na2CO3(s)+ CO2(g)+ H2O(g)Kp = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

For the reaction 2NOCl(g) 2NO(g)+ Cl2(g), Kc = 8.0 at a certain temperature.What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion →\rarr→ greatest completion).

Equilibrium is established for the reaction 2X(s)+ Y(g) 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.

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

The data below refer to the following reaction: 2NO(g)+ Br2(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

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.

What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

The data below refer to the following reaction: 2NO(g)+ Br2(g) 2NOBr(g) Find the concentration of Br2 when the system reaches equilibrium.

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).

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g).What will happen to the mass of carbon if we add gaseous water to the system?

At 340 K, Kp = 69 for the reaction H2(g)+ I2(g) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium?

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?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

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Thermo-Chemistry

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 Orbitals

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Physical Properties of Solutions

Chemical Kinetics

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Acid-Base Equilibria and Solubility Equilibria

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The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq)+ H₂O(l) H₂CO₃(aq) Based on the equilibrium constant reported for this reaction (K_c = 1.70 * 10^-3), there will be more carbon dioxide in solution than carbonic acid.

Sodium carbonate, Na₂CO₃(s), can be prepared by heating sodium bicarbonate, NaHCO₃(s). 2NaHCO₃(s) Na₂CO₃(s)+ CO₂(g)+ H₂O(g)K_p = 0.23 at 100ºC If a sample of NaHCO₃ is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

For the reaction 2NOCl(g) 2NO(g)+ Cl₂(g), K_c = 8.0 at a certain temperature.What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Equilibrium is established for the reaction 2X(s)+ Y(g) 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.

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

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.

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of Br₂ when the system reaches equilibrium.

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).

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).What will happen to the mass of carbon if we add gaseous water to the system?

At 340 K, K_p = 69 for the reaction H₂(g)+ I₂(g) 2HI(g). 50.0 g of HI is injected into an evacuated 5.00-L rigid cylinder at 340 K. What is the total pressure inside the cylinder when the system comes to equilibrium?

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?