An oxidation - reduction in which 3 electrons are transferred has a $\Delta \mathrm{G}^{0}$ of $17.37 \mathrm{~kJ} \mathrm{~mol}^{-1}$ at $25^{\circ} \mathrm{C}$. The value of $\mathrm{E}_{\text {cell }}^{0}$ (in V is \_\_\_\_ $\times 10^{-2}$) $\left(1 \mathrm{~F}=96,500 \mathrm{C} \mathrm{mol}^{-1}\right)$

JEE Main · 2020 · 05 Sep 2020 · Shift 1 · Redox Reactions and Electrochemistry

An oxidation - reduction in which 3 electrons are transferred has a

Δ G^{0}

17.37 kJ mol^{- 1}

2 5^{\circ} C

. The value of

E_{cell}^{0}

(in V is ____

\times 1 0^{- 2}

)

(1 F = 96, 500 C mol^{- 1})

Answer: -6

From

Δ G^{\circ} = - n F E_{cell}^{\circ}

with

Δ G^{\circ} = 17.37 \times 1 0^{3}

J/mol,

n = 3

and

F = 96500

C/mol,

E_{cell}^{\circ} = - \frac{17370}{3 \times 96500} = - 0.06

V. In the units asked for this is

- 6 \times 1 0^{- 2}

V, so the reported value is

- 6

JEE Main · 2020 · 05 Sep 2020 · Shift 1 · Integer answer