For the reaction at equilibrium 2SO3 2SO2 + O2 ($\Delta$Hºrxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will

A) shift to the right. B) shift to the left. C) not shift. D) The question cannot be answered because the equilibrium constant is not given. A) shift to the right. B) shift to the left. C) not shift. D) The question cannot be answered because the equilibrium constant is not given.

Which of these situations will result if some CH4(g)is removed from the reaction CO(g)+ 3H2(g) CH4(g)+ H2O(g)at equilibrium?

A) H2O will be consumed. B) More CH4 and H2O will be produced. C) Kp will decrease. D) More CO will be produced. E) No change will occur. A) H2O will be consumed. B) More CH4 and H2O will be produced. C) Kp will decrease. D) More CO will be produced. E) No change will occur.

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g)+ 1/2O2(g) COCl2(g)+ Cl2(g), Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g)+ O2(g) 2COCl2(g)+ 2Cl2(g).

A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10 A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10

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.

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

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), $\Delta$Hºrxn= 30 kJ/mol

A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume.

Exam 15: Chemical 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. Calculate K_p for the reaction.

(Short Answer)

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Question 61

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 water 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 62

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g), for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

(Multiple Choice)

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Question 63

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)

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Question 64

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H₂(g) $When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H2(g) H2O(g)+ Cu(s) \Delta Hºrxn = -2.0 kJ/mol$ H₂O(g)+ Cu(s) $\Delta$ Hº_rxn = -2.0 kJ/mol

(Multiple Choice)

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Question 65

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].

(True/False)

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Question 66

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) $For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g)+ Br2(g), \Delta Hºrxn = 30 kJ/mol$ 2NO(g)+ Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

(Multiple Choice)

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Question 67

For the reaction at equilibrium 2SO₃ $For the reaction at equilibrium 2SO3 2SO2 + O2 ( \Delta Hºrxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will$ 2SO₂ + O₂ ( $\Delta$ Hº_rxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will

(Multiple Choice)

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Question 68

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.

(True/False)

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Question 69

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 Cu²⁺(aq)+ 4CN^-(aq) Cd(CN)₄^2-(aq)K_c = 1.0 * 10²⁵ What will be the concentration of CN^-(aq)at equilibrium?

(Essay)

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Question 70

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 71

Which of these situations will result if some CH₄(g)is removed from the reaction CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)at equilibrium?

(Multiple Choice)

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Question 72

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). Which way will the reaction shift if the pressure on the system is increased?

(Short Answer)

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Question 73

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g)+ ¹/₂O₂(g) COCl₂(g)+ Cl₂(g), K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g)+ O₂(g) 2COCl₂(g)+ 2Cl₂(g).

(Multiple Choice)

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Question 74

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.

(True/False)

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Question 75

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 76

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide. CaCO₃(s) CaO(s)+ CO₂(g) K_P for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO₃(s)was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume occupied by the solid, what will be the overall mass percent of carbon in the solid once equilibrium is reached?

(Short Answer)

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Question 77

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 78

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase? 2NOBr(g) $For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), \Delta Hºrxn= 30 kJ/mol$ 2NO(g)+ Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

(Multiple Choice)

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Question 79

For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) $For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) 2NO(g)+ Br2(g), \Delta Hºrxn = 30 kJ/mol$ 2NO(g)+ Br₂(g), $\Delta$ Hº_rxn = 30 kJ/mol

(Multiple Choice)

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Question 80

Showing 61 - 80 of 99

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. Calculate K_p for the reaction.

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 water 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.

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g), for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

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

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.

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

Which of these situations will result if some CH₄(g)is removed from the reaction CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)at equilibrium?

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). Which way will the reaction shift if the pressure on the system is increased?

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g)+ ¹/₂O₂(g) COCl₂(g)+ Cl₂(g), K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g)+ O₂(g) 2COCl₂(g)+ 2Cl₂(g).

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

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Exam 15: Chemical 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. Calculate Kp for the reaction.

Kc for the reaction CO2(g)+ H2(g) H2O(g)+ CO(g)is 1.6 at about 990ºC. Calculate the number of moles of water 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.

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g)+ I2(g), for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H2 at equilibrium.

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

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H2(g) H2O(g)+ Cu(s) Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

The equilibrium constant expression for the reaction CuO(s)+ H2(g) Cu(s)+ H2O(g)is Kc = [H2]/[H2O].

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g)+ Br2(g), Δ\DeltaΔ Hºrxn = 30 kJ/mol

For the reaction at equilibrium 2SO3 2SO2 + O2 ( Δ\DeltaΔ Hºrxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will

For the reaction H2(g)+ I2(g) 2HI(g), KP = Kc.

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 Cu2+(aq)+ 4CN-(aq) Cd(CN)42-(aq)Kc = 1.0 * 1025 What will be the concentration of CN-(aq)at equilibrium?

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

Which of these situations will result if some CH4(g)is removed from the reaction CO(g)+ 3H2(g) CH4(g)+ H2O(g)at equilibrium?

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g). Which way will the reaction shift if the pressure on the system is increased?

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g)+ 1/2O2(g) COCl2(g)+ Cl2(g), Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g)+ O2(g) 2COCl2(g)+ 2Cl2(g).

When the reaction 2O3(g) 3O2(g), for which Kp = 3.0 * 1026 at 773ºC, is at equilibrium, the mixture will contain very little O2 as compared to O3.

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), Δ\DeltaΔ Hºrxn= 30 kJ/mol

For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) 2NO(g)+ Br2(g), Δ\DeltaΔ Hºrxn = 30 kJ/mol

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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. Calculate K_p for the reaction.

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 water 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.

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g), for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

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

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.

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

Which of these situations will result if some CH₄(g)is removed from the reaction CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)at equilibrium?

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). Which way will the reaction shift if the pressure on the system is increased?

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g)+ ¹/₂O₂(g) COCl₂(g)+ Cl₂(g), K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g)+ O₂(g) 2COCl₂(g)+ 2Cl₂(g).

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.