Chapter 6, Problem 6.44P

Interpretation Introduction

Interpretation:

The unknown volume of water at $18.2°\text{C}$ that is added to $24.4\text{ mL}$ of water at $35.0°\text{C}$ to get the final temperature $23.5°\text{C}$ 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:

$q=\left(\text{mass}\right)\left(c\right)\left(\Delta T\right)$        (1)

Here,

$\Delta T$ is the temperature difference.

$q$ is the heat released or absorbed.

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

The formula to calculate the mass of a substance is as follows:

$\text{mass}=\left(\text{density}\right)\left(\text{volume}\right)$        (2)