Consider the following redox reaction taking place in acidic medium
$
\mathrm{BH}_4^{-}(a q)+\mathrm

Question

Consider the following redox reaction taking place in acidic medium
$
\mathrm{BH}_4^{-}(a q)+\mathrm{ClO}_3^{-}(a q) \longrightarrow \mathrm{H}_2 \mathrm{BO}_3^{-}(a q)+\mathrm{Cl}^{-}(a q)
$
If the Nernst equation for the above balanced reaction is
$
\mathrm{E}_{\mathrm{cell}}=\mathrm{E}_{\mathrm{cell}}^{\circ}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \mathrm{Q},
$
then the value of $n$ is $\_\_\_\_$ .(Nearest integer)

Professor PC Thomas Classes · Answer

See detailed solution for explanation.