Question

Determine the value of the equilibrium constant for the reaction

$2Br^{-}\left(\right.aq\left.\right)+I_{2}\left(\right.s\left.\right) \rightleftharpoons Br_{2}\left(\right.l\left.\right)+2I^{-}\left(\right.aq\left.\right)$

$E_{c e l l}^{o}=-0.54\text{V}$

• A. $5.01\times 10^{- 19}$
• B. 18.30
• C. $1.7\times 10^{54}$
• D. $1.9\times 10^{18}$

Answer 1

Answer: (A)

The relation between equilibrium constant (K) and $E_{c e l l}^{o}$ is given as

$log K=\frac{E_{c e l l}^{o} . n}{0.059 \text{V}}$

here, n = 2

$=\frac{- 0.54 \text{V} \times 2}{0.059 \text{V}}$

$=\frac{- 1.08}{0.059}=-18.3$

On taking antilog

$K=5.01\times 10^{- 19}$