(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

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, Problem 6.8P

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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There is an instrument in Johnson 334 that measures total-reflectance x-ray fluorescence (TXRF) to do elemental analysis (i.e., determine what elements are present in a sample). A researcher is preparing a to measure calcium content in a series of well water samples by TXRF with an internal standard of vanadium (atomic symbol: V). She has prepared a series of standard solutions to ensure a linear instrument response over the expected Ca concentration range of 40-80 ppm. The concentrations of Ca and V (ppm) and the instrument response (peak area, arbitrary units) are shown below. Also included is a sample spectrum. Equation 1 describes the response factor, K, relating the analyte signal (SA) and the standard signal (SIS) to their respective concentrations (CA and CIS). Ca, ppm V, ppm SCa, arb. units SV, arb. units 20.0 10.0 14375.11 14261.02 40.0 10.0 36182.15 17997.10 60.0 10.0 39275.74 12988.01 80.0 10.0 57530.75 14268.54 100.0…

A mixture of 0.568 M H₂O, 0.438 M Cl₂O, and 0.710 M HClO are enclosed in a vessel at 25 °C. H₂O(g) + C₁₂O(g) = 2 HOCl(g) K = 0.0900 at 25°C с Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C₁₂O]= [HOCI]= M Σ M

What units (if any) does the response factor (K) have? Does the response factor (K) depend upon how the concentration is expressed (e.g. molarity, ppm, ppb, etc.)?

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, Problem 6.8P

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, Problem 6.8P

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 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, Problem 6.8P

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, Problem 6.8P

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, Problem 6.8P

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, Problem 6.8P

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 11

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Answer 12

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Answer 13

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