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

Calculate ΔH° for each reaction. a. HO• + CH4 → •CH3 + H2O b. CH3OH + HBr → CH3Br + H2O

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 5.7, Problem 25P

(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

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

Calculate ΔH° for each reaction. a. HO• + CH4 → •CH3 + H2O b. CH3OH + HBr → CH3Br + H2O

Consider the following reaction: 4 FeS2 (s) + 11 O2 (g) ↔ 2 Fe2O3 (s) + 8 SO2 (g) What is true about this process? A. ΔH > 0 and the reactants are energetically favored B. ΔH < 0 and the reactants are energetically favored C. ΔH < 0 and the products are energetically favored D. ΔH > 0 and the products are energetically favored

Calculate ΔH° for the reaction using the given bond dissociation energies. CH4(g)+2O2(g)⟶CO2(g)+2H2O(g) Bond ΔH° (kJ/mol) O–OO–O 142 H–OH–O 459 C−HC−H 411 C=OC=O 799 O=OO=O 498 C–OC–O 358 What type of reaction is this?

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 5.7, Problem 25P

(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

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

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 5.7, Problem 25P

(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

Trending nowThis is a popular solution!

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 5.7, Problem 25P

(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

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Answer 5

Chapter 5.7, Problem 25P

(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 5.7, Problem 25P

(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 5.7, Problem 25P

(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

Expert Solution & Answer

Answer 15

Expert Solution & Answer

Answer 16

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Answer 17

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Answer 18

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Answer 19

Trending nowThis is a popular solution!

Answer 20

Trending nowThis is a popular solution!

Answer 21

Trending nowThis is a popular solution!

Answer 22

Trending now

Answer 23

This is a popular solution!

Answer 24

See solution

Check out sample textbook solution

Answer 25

Ch. 5.1 - Determine the degree of unsaturation and then draw...Ch. 5.1 - Prob. 4P Ch. 5.2 - Prob. 5P Ch. 5.2 - Draw the structure for each of the following: a....Ch. 5.2 - What is each compounds systematic name?Ch. 5.4 - Assign relative priorities to each set of...Ch. 5.4 - Tamoxifen slows the growth of some breast tumors...Ch. 5.4 - Draw and label the E and Z isomers for each of the...Ch. 5.4 - Prob. 12P Ch. 5.4 - Name each of the following:

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

Concept explainers

Chapter 5 Solutions