Chapter 5, Problem 28QP

Interpretation Introduction

Interpretation:

The heat released in the formation of $1.26\times {10}^4\text{g}$ of nitrogen dioxide in the given reaction is to be calculated.

Concept Introduction:

Sign of enthalpy change depends upon the heat change of the system. If the system involves absorption of heat, then the sign of enthalpy change is positive, and if the system involves release of heat, then the sign of enthalpy change is negative.

The enthalpy change associated with the given mass of compound is calculated by the formula,

$\Delta \text{H}=\frac{\text{Moles}\text{of}\text{compound}\text{in}\text{the}\text{system}\times \text{Enthalpy}\text{change}\text{of}\text{the}\text{reaction}}{\text{Moles}\text{of}\text{compound}\text{in}\text{thermochemical}\text{equation}}$

$\text{Moles of}\text{compound}=\frac{\text{Mass}\text{of}\text{Compound}}{\text{Molar}\text{mass}\text{of}\text{Compound}}$