Chapter 12, Problem 90E

Interpretation Introduction

Interpretation:

For the total loss of energy by a body from eating $145\text{ g}$ 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 $\text{Δ}{H}_{\text{fus}}$.

For 1 mole of ice, $\text{Δ}{H}_{\text{fus}}$ is equal to $6.02\text{ kJ}$ 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.

$1\text{ J}=0.239\text{ cal}$(calories).

One nutritional Calorie is represented by capital “C” Calories and $1000\text{ cal}=1\text{ C}$.