Chapter 5, Problem 5.69QP

(a)

Interpretation Introduction

Interpretation: The addition of $2.00\text{g}$ of $\text{Mg}$ metal in $95.0\text{mL}$ of $1.00\text{M}$ of $\text{HCl}$ in a coffee-cup calorimeter raised the temperature by $9.2°\text{C}$. The balanced net ionic equation of the reaction is to be written and $\Delta H_{\text{rxn}}$ is to be calculated.

Concept introduction: The heat of reaction or enthalpy of the reaction $\left(\Delta H_{\text{rxn}}\right)$ is defined as the amount of energy released or absorbed during formation of product. It is calculated by formula,

$q=n\times c_{\text{p}}\times \Delta T$

To determine: The balanced net ionic equation of the reaction.

(b)

Interpretation Introduction

To determine: The enthalpy of the reaction $\Delta H_{\text{rxn}}$.