Chapter 13, Problem 26PE

Interpretation Introduction

Interpretation:

Energy removed from $325\text{ g}$ of water at $35°\text{C}$ to convert into ice at $0°\text{C}$ has to be calculated.

Concept Introduction:

Heat required by $\text{1 g}$ of a substance to increase the temperature by $1°\text{C}$ is termed as specific heat capacity of that substance. Energy absorbed or released by the substance is calculated as follows:

  $\text{Energy}=\left(\text{mass}\right)\left(\text{specific heat}\right)\left(\text{change in temperature}\right)$

Heat of fusion is the quantity of heat required to convert liquid to solid. Every substance has different heat of fusion. Heat of fusion for water is $333.55\text{ J/g}$. It is represented as ${\text{ΔH}}_{\text{fus}}$ and calculated as follows:

  $\text{q}=\left(\text{mass}\right)\left({\text{ΔH}}_{\text{fus}}\right)$