To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions. Concept Introduction: Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction. Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy ( ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS) . Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas. Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

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Answer 1

Question

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

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Answer 2

Question

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

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Answer 3

Question

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

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Answer 4

Question

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

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Answer 5

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 6

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 7

Chapter 15, Problem 15.45QP

(a)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 8

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 9

(b)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 10

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 11

(c)

Interpretation Introduction

Interpretation:

To predict the change of equilibrium constant (Kc) given set of endothermic and exothermic equilibrium reactions.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy (ΔH) of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation G=H-(TS) or (ΔG=ΔH-TΔS).

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. These type of chemical reactions that is accompanied by the absorption of heat.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 15.1 - Review of Concepts Consider the equilibrium X ⇌ Y,...Ch. 15.2 - Practice Exercise Write Kc and Kp for the...Ch. 15.2 - Practice Exercise For the reaction N2(g) + 3H2(g)...Ch. 15.2 - Practice Exercise Consider the following...Ch. 15.2 - Prob. 1RC Ch. 15.2 - Prob. 2RC Ch. 15.3 - Practice Exercise The equilibrium constant (Kc)...Ch. 15.3 - Prob. 1RC Ch. 15.3 - Practice Exercise Consider the reaction in Example...Ch. 15.3 - Practice Exercise At 1280°C the equilibrium...

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