If the $\Delta G$ of a cell reaction ${\rm{AgCl}} + {e^ - } \to {\rm{Ag}} + {\rm{C}}{{\rm{l}}^ - }$ is $ - 21.20$ kJ, the standard emf of cell is

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

1 Hard

1 of 1

Application +4 | -1

If the

\Delta G

of a cell reaction

\mathrm{AgCl} + {e^ - } \to \mathrm{Ag} + \mathrm{C}{\mathrm{l}^ - }

- 21.20

kJ, the standard emf of cell is

View answer and explanation

Correct option: B

0.220 V

Option B (0.220 V) is correct because it is calculated using the relationship between Gibbs free energy and standard EMF:

E^0 = -\frac{{\Delta G}}{{nF}}

Practice All Chapter MCQs →

A{l^{3 + }}

{H_2}

{H^ + }

\mathrm{LiCl},{\rm{NaCl {\kern 1pt}{\kern 1pt}and {\kern 1pt}{\kern 1pt}KCl}}

\left(\mathrm{CuSO}_4\right)

\mathrm{A}{\mathrm{l}^{3 + }}