Chapter 22, Problem 22.84QP

Interpretation Introduction

Interpretation:

Volume of ${\text{Cl}}_{\text{2}}$ gas in litres that is required to oxidize bromide to molecular bromine in a water tank has to be calculated.

Concept Introduction:

Oxidation is the reaction in which electrons are liberated or released from a chemical species.

Reduction is the reaction in which electrons are consumed by a chemical species.

In this problem, bromide ion has been oxidized into bromine molecule using chlorine gas.

Bromide ion releases electrons on oxidation which are taken up by the chlorine gas. Hence, the conversion of bromide ion into bromine molecule is carried out by the reduction of chlorine gas.

The overall reaction can be given as follows:

${\text{2Br}}^{\text{-}}\left(\text{aq}\right)\text{+}{\text{Cl}}_{\text{2}}\left(\text{g}\right)\stackrel{}{\to }{\text{2Cl}}^{\text{-}}\left(\text{aq}\right)\text{+}{\text{Br}}_{\text{2}}\left(\text{l}\right)$

The volume of chlorine gas required for the bromide oxidation in the water tank can be calculated using the idea gas equation as shown here:

The ideal gas equation is $\text{PV}\text{=}\text{nRT}$

$\text{V}\text{=}\frac{\text{nRT}}{\text{P}}$

Where,

$\text{n}$ is the number of moles of the gas.

$\text{R}$ is the gas constant.

$\text{P}$ is the pressure.

T is the temperature.