Chapter 13, Problem 13.27P

Interpretation Introduction

Interpretation:

The quantities that must be nearly equal in magnitude for small value of $\Delta H_{\text{solution}}$. Also, whether their signs will be the same or opposite is to be determined.

Concept introduction:

The enthalpy is the thermodynamic property of the system. It is defined as the sum of internal energy and the product of pressure and volume of the system. It is a state function and is independent of the path followed by the system from initial to the final state. It is an extensive property. The total enthalpy of the system cannot be measured directly so the change in enthalpy $\left(\Delta H\right)$ is measured. If $\Delta H$ of the reaction is positive, it is an endothermic reaction and if $\Delta H$ of the reaction is negative, it is an exothermic reaction.

The enthalpy change of solution is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by $\Delta H_{\text{solution}}$. It can either be positive or negative.