(a) Interpretation: The ΔH° value for the given oxidation reaction is to be calculated. Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH° . Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

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Answer 1

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Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

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To a test tube containing 5.0 ml of 1.00 M NaOH at 27°C in a calorimeter, 5.0 ml of 2.00 M HNO3 at the same temperature was added, the heat generated by the reaction was monitored. Which of the following is TRUE? a.Reaction is exothermic; solution will turn pink upon addition of phenolphthalein. b.Heat is absorbed by the system; no color change will be observed upon addition of phenolphthalein. c.Heat is released by the system; no color change will be observed upon addition of phenolphthalein. d.Reaction is endothermic; solution will turn pink upon addition of phenolphthalein.

Consider the following reaction:2CH3OH(g)→2 CH4(g) + O2(g) H=+252.8 kJ a. Is this reaction exothermic or endothermic? Explain briefly. b. Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure c. For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane, CH4, are produced? d. How many kilojoules of heat are released when 38.5 g of CH4 (g) reacts completely with O2 (g) to form CH3OH( g) at constant pressure?

22. Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong base) is always -55.90 kJ per mole of H2O formed, what is the concentration of a 65 mL sample of HCl if the enthalpy of neutralization for the reaction was found to be -5.38 kJ, assuming no heat is lost to the calorimeter? 0.96 M 1.48 M 1.60 M 0.38 M 4.63 M

Answer 2

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

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Answer 3

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Expert Solution & Answer

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Answer 4

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

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Answer 5

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Answer 6

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Answer 7

Chapter 6.4, Problem 8P

Interpretation Introduction

(a)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products are known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Answer 8

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Answer 9

Interpretation Introduction

(b)

Interpretation: The ΔH° value for the given oxidation reaction is to be calculated.

Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Answer 10

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Answer 12

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Answer 13

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