Chapter 19, Problem 19.133MP

(a)

Interpretation Introduction

Interpretation:

The balanced equation for the given reaction has to be given.

Concept introduction:

In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.

Coefficient is a number placed before a formula in a chemical equation.

A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.

(b)

Interpretation Introduction

Interpretation:

The volume of gas in litres produced from the explosion of $1.80m^3$ of solid $N{H}_{4}N{O}_3$ has to be calculated.

Concept introduction:

Ideal gas Equation:

Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.

$\begin{array}{l}\text{V }\propto \frac{\text{nT}}{\text{P}}\\ \text{V = R}\frac{\text{nT}}{\text{P}}\\ \text{PV = nRT}\end{array}$

Where,

$\begin{array}{l}\text{n = moles}\text{of}\text{gas}\\ \text{P = pressure}\\ \text{T = temperature}\\ \text{R = gas }\text{constant}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The amount of heat in kilojoules released in the reaction has to be determined.

Concept introduction:

Standard heat of reaction:

The value of standard heat energy change ${\text{ΔH}}^{\text{ο}}$ of the given reaction is calculated by the formula,

${\text{ΔH}}^{\text{ο}}\text{=}{{\displaystyle \sum {\text{ΔH}}_{\text{f}}^{\text{ο}}}}_{\left(\text{products}\right)}-{{\displaystyle \sum {\text{ΔH}}_{\text{f}}^{\text{ο}}}}_{\left(\text{reactants}\right)}$

Where,

$\begin{array}{c}{\text{ΔH}}_{\text{f}}^{\text{ο}}{}_{\left(\text{reactants}\right)}\text{=}\text{the enthalpy of formation for the reactants}\\ {\text{ΔH}}_{\text{f}}^{\text{ο}}{}_{\left(\text{products}\right)}\text{=}\text{the enthalpy of formation for the products}\end{array}$