The standard free energy change of reaction 2Fe2+(aq)+Cl2(g)⟶2Fe3+(aq)+2Cl−(aq) is −114.0 kJ mol−1. The standard emf of the cell producing this reaction will be about

The standard free energy change of reaction $2 {Fe}^{2 +} (aq) + {Cl}_{2} (g) ⟶ 2 {Fe}^{3 +} (aq) + 2 {Cl}^{-} (aq)$ is $- 114.0 kJ {mol}^{- 1}$ . The standard $e m f$ of the cell producing this reaction will be about

A
$0.59 V$
B
$0.65 V$
C
$0.42 V$
D
$- 0.23 V$

Solution:

For the given reaction, $n = 2$ .

Hence,

$E^{\circ} = - \frac{Δ_{r} G^{\circ}}{n F} = \frac{114.0 \times 10^{3} J {mol}^{- 1}}{(2) (96500 C {mol}^{- 1})} = 0.59 V$

Thus, the correct option is A.

Related content

Distance Speed Time Formula

Refractive Index Formula

Mass Formula

Electric Current Formula

Ohm’s Law Formula

Wavelength Formula

Electric Power Formula

Resistivity Formula

Weight Formula

Linear Momentum Formula