Chapter 8, Problem 8.126CHP

Interpretation Introduction

Interpretation:

An experiment involves measuring the temperature change in the reaction of $100\text{ mL}$ of $0.200M$ $CsOH$ with $50\text{ mL}$ of $0.400M$ $HCl.$  $\Delta H$ for the reaction has to be calculated in kilojoules.

Concept Introduction:

Specific heat is the heat required to raise the temperature of $1g$ of a substance by accurately $1°C.$

Specific heat is denoted by ‘c’ and the formula is,

$c=\frac{q}{m\times \Delta T}$

Where,

$\begin{array}{l}q=quantity\text{ of heat added}\\ \Delta T=change\text{ in temperature}\\ \text{m}\text{= mass of the substance}\end{array}$

$\Delta H$ refers to change in enthalpy.

Heat liberated or absorbed during the reaction is,

$q=\Delta H\times n$

Where,

$q=heat\text{ liberated or absorbed}\text{. n = no}\text{.of moles of the substance}$

If sign of ‘q’ is negative it implies heat is liberated.  If sign of ‘q’ is positive it implies heat is absorbed.