Chapter 3, Problem 3.69P

(a)

Interpretation Introduction

Interpretation:

The moles of ${\text{Cl}}_2$ produced by the reaction of $1.82\text{ mol}$ of $\text{HCl}$ with excess ${\text{MnO}}_2$ is to be calculated.

Concept introduction:

In a balanced chemical equation, the total mass of reactants and products are equal in a balanced chemical equation, thus, it obeyed the law of conservation of mass. Also, the amounts of substances in a balanced chemical reaction are stoichiometrically equivalent to each other.

A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction.

(b)

Interpretation Introduction

Interpretation:

The mass of ${\text{Cl}}_2$ produced by the reaction of $1.82\text{ mol}$ of $\text{HCl}$ with excess ${\text{MnO}}_2$ is to be calculated.

Concept introduction:

In a balanced chemical equation, the total mass of reactants and products are equal in a balanced chemical equation, thus, it obeyed the law of conservation of mass. Also, the amounts of substances in a balanced chemical reaction are stoichiometrically equivalent to each other.

The expression to calculate the mass from the moles of a substance is as follows:

$\text{Mass}\left(\text{g}\right)=\left(\text{Amount}\left(\text{mol}\right)\right)\left(\text{Molar mass}\left(\text{g/mol}\right)\right)$