Chapter 12, Problem 12.19P

Interpretation Introduction

Interpretation:

The total heat that is needed to convert $22.00\text{ g}$ of ice at $-6.00°\text{C}$ to liquid water at $0.500°\text{C}$ is to be calculated.

Concept introduction:

Specific heat capacity $\left(c\right)$ of a substance is the amount of heat needed to raise the temperature of $1\text{g}$ of a substance by $1\text{K}$. The formula to calculate heat required is as follows:

$q=\left(\text{mass}\right)\left(c\right)\left(T_2-T_1\right)$ (1)

Here,

$T_2$ is the final temperature.

$T_1$ is the initial temperature.

$q$ is the heat released or absorbed.

$c$ is the specific heat capacity of the substance.

The formula to calculate heat at phase change is as follows:

$q=\left(\text{mol}\right)\left(\Delta H\right)$ (2)

Here,

$\Delta H$ is the enthalpy change.