The value of ΔH 0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy. Concept introduction: The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken. ΔH 0 = Heat required to break bonds - Heat released from forming bonds Heat is one form of energy. The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

Question

1) Suppose 0.1 kg ice at 0°C (273K) is in 0.5kg water at 20°C (293K). What is the change in entropy of the ice as it melts at 0°? To produce the original "water gas" mixture, carbon (in a combustible form known as coke) is reacted with steam: 131.4 kJ + H20(g) + C(s) → CO(g) + H2(g) From this information and the equations in the previous problem, calculate the enthalpy for the combustion or carbon to form carbon dioxide. kindly show me how to solve both parts of the same long problem. Thanks

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 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

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1) Suppose 0.1 kg ice at 0°C (273K) is in 0.5kg water at 20°C (293K). What is the change in entropy of the ice as it melts at 0°? To produce the original "water gas" mixture, carbon (in a combustible form known as coke) is reacted with steam: 131.4 kJ + H20(g) + C(s) → CO(g) + H2(g) From this information and the equations in the previous problem, calculate the enthalpy for the combustion or carbon to form carbon dioxide. kindly show me how to solve both parts of the same long problem. Thanks

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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 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Expert Solution & Answer

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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 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Expert Solution & Answer

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See solution

Check out sample textbook solution

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 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Expert Solution & Answer

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Check out sample textbook solution

Answer 5

Chapter 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Answer 6

Chapter 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

Answer 7

Chapter 5.8, Problem 23P

(a)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of HCl to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The value of ΔH0 for the addition of H2 to ethene should be determined using bond dissociation enthalpy.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

Answer 10

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

Answer 11

(c)

Interpretation Introduction

Interpretation:

It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

A reaction with a negative ΔH0 is called an exothermic reaction.

A reaction with a positive ΔH0 is called an endothermic reaction.

Answer 12

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Answer 13

(d)

Interpretation Introduction

Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.

Concept introduction:

The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.

ΔH0 = Heat required to break bonds - Heat released from forming bonds

Heat is one form of energy.

The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.

The mathematical relationship between enthalpy (H) and free energy (G) is,

ΔG0 = ΔH0- TΔS

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Answer 14

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Ch. 5.1 - What is the molecular formula for each of the...Ch. 5.1 - Prob. 4P Ch. 5.1 - Determine the degree of unsaturation and then draw...Ch. 5.1 - Prob. 6P Ch. 5.2 - What is each compounds systematic name?Ch. 5.2 - Prob. 8P Ch. 5.2 - Draw the structure for each of the following: a....Ch. 5.3 - How many carbons are in the planar double-bond...Ch. 5.3 - Prob. 12P Ch. 5.5 - Prob. 13P

Solution Summary: The author explains the bond dissociation enthalpy, which determines the value of HCl to ethene.

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