Chapter 14, Problem 14.20P

Interpretation Introduction

Interpretation:

Solubility of ${\text{Br}}_{\text{2}}\left(aq\right)$ in $\text{g/L}$ has to be calculated.

Concept Introduction:

Cell that is more negatively charged has better oxidation tendency and thus will readily lose electron. Electrons released from this electrode will reach positively charged reduction potential electrode.

Expression to compute $K$ from cell potential as per the Nernst equation as follows:

  $K={10}^{n(E_{\text{cell}}^{°})/0.05916}$

Here,

$K$ denotes equilibrium constant.

$E_{\text{cell}}^{°}$ denotes standard cell potential.

$n$ denotes moles of electrons transferred.