Chapter 6, Problem 6.48P

Interpretation Introduction

Interpretation:

$\Delta H$ of $\text{AgCl}$ formed when $20.0\text{ mL}$ of $0.200M{\text{ AgNO}}_3$ and $30.0\text{ mL}$ of $1.00M\text{ NaCl}$ are mixed in a coffee-cup calorimeter at $24.72°\text{C}$ is to be calculated.

Concept introduction:

Specific heat capacity $\left(c\right)$ of a substance is the amount of the 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.

At the constant pressure the value of $q_{\text{p}}$ is equal to $\Delta H$.