Chapter 5.4, Problem 5.12BFP

Interpretation Introduction

Interpretation:

The volume of hydrogen gas at $765\text{ torr}$ and $225°\text{C}$ required to reduce $35.5\text{ g}$ of $\text{copper}\left(\text{II}\right)\text{oxide}$.

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 formula to calculate the moles is,

  $\text{Moles}=\frac{\text{given mass}}{\text{molar mass}}$        (1)

The ideal gas equation can be expressed as follows:

  $PV=nRT$        (2)

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.