Mass difference of the given reaction has to be calculated Concept Introduction: Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy. Change in mass of a given reaction can be determined as given, Δ m = M a s s of reactant − Mass of products

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Answer 1

Question

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

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Answer 2

Question

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

Answer 6

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Answer 7

Chapter 24, Problem 24.93P

(a)

Interpretation Introduction

Interpretation:

Mass difference of the given reaction has to be calculated

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Change in mass of a given reaction can be determined as given,

$Δm = Mass of reactant− Mass of products$

Answer 8

(a)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass of products:

Mass of products is determined as shown below,

$Mass of products = Mass of 24He + Mass of 94239Pu= (4.0026 amu)+(239.0522 amu)= 243.0548 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= 0.0066 amu$

Mass difference is $0.0066 amu$ .

Convert unit of mass difference to $Kg$ :

Mass difference for the reaction is converted from $amu to kg$ as follows,

$Δm = (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

Answer 13

(b)

Interpretation Introduction

Interpretation:

Energy released (in $J$ )during the given reaction has to be determined.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

Answer 14

(b)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released is calculated as follows for the reaction,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10-13 J.$

Answer 15

(b)

Expert Solution

Answer 16

(b)

Expert Solution

Answer 17

Expert Solution

Answer 18

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.

Answer 19

(c)

Interpretation Introduction

Interpretation:

Energy released (in $kJ/mol$ )during the given reaction has to be determined and difference between this energy values of heat of energy in a chemical reaction has to be commented.

Concept Introduction:

Nuclear reaction: A nuclear reaction in which a lighter nucleus fuses together into new stable nuclei or a heavier nucleus split into stable daughter nuclei with the release of large amount of energy.

Nuclear binding energy: It is the energy that requires for the breaking one mole of nuclei of an element to its individual nucleons.

$Nucleus + nuclear binding energy → nucleons$

It can be calculated using the given formula,

$ΔE = Δmc2where,Δm = Mass Differencec= Speed of light$

Answer 20

(c)

Expert Solution

Explanation of Solution

Given information is shown below,

$Given reaction: 96243Cm→ 94239Pu+ 24HeMass of 96243Cm= 243.0614 amuMass of 94239Pu= 239.0522 amuMass of 24He= 4.0026 amu$

Calculate the mass difference:

Mass of reactants $(96243Cm)$ is $243.0614 amu$

Mass difference of the reaction can be calculated as given,

$Δm = Mass of reactant− Mass of products= (243.0614 amu)−(243.0548 amu)= (0.0066 amu)(1.661×10−24 g1 amu)(1 kg10−3 kg)= 1.1×10−29 kg$

Mass difference for the reaction is $1.1×10−29 kg$ .

Calculate the energy released:

Energy released for the reaction is calculated as follows,

$Energy released, E = mc2= (1.1×10−29 kg)(2.998×108 m/s)2= 9.8527×10−13 J$

Energy released during the given reaction is $9.8527×10−13 J.$

Convert the unit of energy released to $kJ/mol$ :

Unit of energy released is converted as follows,

$Binding energy, E in kJ/mol = (9.8527×10−13 Jreactions)(6.022×1023 reactions1Emol)(1 kJ103 J)= 5.9×108 kJ/mol$

Energy released during the given reaction is $5.9×108 kJ/mol$ .

Energy released during the given reaction is $5.9×108 kJ/mol$ whereas the energy values of heat of energy in a chemical reaction are in few hundreds $kJ/mol$ .

This value is about one million times more than a typical heat of energy in a chemical reaction.