For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined. Concept introduction: The heat of fusion is the amount of heat required to melt 1mol of a solid. It is denoted by Δ H fus . For 1 mole of ice, Δ H fus is equal to 6.02 kJ at the freezing point of water. Number of moles is equal to the mass of species divided by its molar mass. A thousand of joules is one kilojoule. 1 J = 0.239 cal (calories). One nutritional Calorie is represented by capital “C” Calories and 1000 cal = 1 C .

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Answer 1

Question

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

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Answer 2

Question

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

Expert Solution & Answer

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Answer 3

Question

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

Expert Solution & Answer

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Answer 4

Question

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

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Answer 5

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

Answer 6

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

Answer 7

Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating 145 g of ice in joules, kilojoules, calories and nutritional Calories is to be determined.

Concept introduction:

The heat of fusion is the amount of heat required to melt 1mol of a solid.

It is denoted by ΔHfus.

For 1 mole of ice, ΔHfus is equal to 6.02 kJ at the freezing point of water.

Number of moles is equal to the mass of species divided by its molar mass.

A thousand of joules is one kilojoule.

1 J=0.239 cal(calories).

One nutritional Calorie is represented by capital “C” Calories and 1000 cal=1 C.

Answer 8

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Answer 9

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Answer 10

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Answer 11

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