The amount of heat released when 0.255 m o l of aluminum has reacted in k J is to be determined. Concept Introduction: Enthalpy H : it is the total amount of heat in a particular system. The value of heat formed in a reaction ΔH is calculated by the formula, ΔH= ∑ ( B o n d D i s s o c i a t i o n E n e r g y ) ( reactants ) − ∑ ( B o n d D i s s o c i a t i o n E n e r g y ) ( products ) If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction. Conversion of k c a l to joules is 1 k c a l = 4184 J

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Answer 1

Question

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

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Answer 2

Question

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Expert Solution & Answer

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Answer 4

Question

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Answer 6

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

Answer 7

Chapter 7, Problem 7.76CP

(a)

Interpretation Introduction

Interpretation:

The amount of heat released when $0.255 mol$ of aluminum has reacted in $kJ$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

Answer 8

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Answer 9

(b)

Interpretation Introduction

Interpretation:

The amount of heat released when $5 g$ of aluminum has reacted in $kcal$ is to be determined.

Concept Introduction:

Enthalpy $H$ : it is the total amount of heat in a particular system.

The value of heat formed in a reaction $ΔH$ is calculated by the formula,

$ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)$

If the value obtained for $ΔH$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $ΔH$ is negative it is an exothermic reaction.

Conversion of $kcal$ to joules is $1 kcal = 4184 J$

From its given mass is,

$Number of moles = Given massMolecular mass$

Answer 10

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Answer 11

Expert Solution & Answer

Answer 12

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Answer 13

Ch. 7.1 - Classify each of the following as having potential...Ch. 7.2 - Based on bond energies, which atmospheric gas in...Ch. 7.3 - Prob. 7.1CIAP Ch. 7.3 - How many Calories (i.e., kilocalories) are in a...Ch. 7.3 - Prob. 7.3P Ch. 7.3 - Prob. 7.4P Ch. 7.3 - Prob. 7.5P Ch. 7.3 - Prob. 7.6P Ch. 7.4 - Prob. 7.7P Ch. 7.4 - Prob. 7.8KCP

Solution Summary: The author explains that the amount of heat released when 0.255mol of aluminum has reacted in kJ is to be determined.

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