Chapter 5.5, Problem 5.11E

Interpretation Introduction

Interpretation:

The number of moles of oxygen that would be obtained from 1.300 g of ${\text{KClO}}_{\text{3}}$ has to be calculated.

The volume of oxygen collected over water at ${\text{23}}^{\circ }\text{C}$ and at a total pressure of 745 mmHg has to be calculated.

Concept Introduction:

Partial Pressure:

Dalton’s law of partial pressure states that “the total pressure (P) of the mixture is equal to the sum of the partial pressures ${\text{(P}}_{\text{A}}{\text{, P}}_{\text{B}}{\text{, P}}_{\text{C}}\mathrm{.....}\text{)}$ of all the component gases $\text{(A, B, C}\mathrm{......}\text{)}$  present in the mixture” and is given as,

${\text{P = P}}_{\text{A}}{\text{ + P}}_{\text{B}}{\text{ + P}}_{\text{C}}\text{ + }\mathrm{.......}$

The ideal gas law for the individual gas component A is given as,

${\text{P}}_{\text{A}}{\text{V = n}}_{\text{A}}\text{RT}$

Collection of gas over water:

When gases are collected over water, the partial pressure of water vapor depends only on the temperature and this partial pressure is known as the vapor pressure of water.