Question

If for the given reaction taking place at $25^\circ C$ in a cell is,

$\frac{1}{2} \text{Cu} \left(\text{s}\right) + \frac{1}{2} \left(\text{Cl}\right)_{2} \left(\text{g}\right) \rightarrow \frac{1}{2} \left(\text{Cu}\right)^{2 +} + \left(\text{Cl}\right)^{-}$

having standard e.m.f. of $1.02 \, volts$ . Calculate standard free energy change.

• A. $-98430$ $J$
• B. $98430$ $J$
• C. $96500$ $J$
• D. $-96500$ $J$

Answer 1

Answer: (A)

The relation between free energy change and standard e.m.f. is given by $\Delta G=-nFE^\circ $

$\Delta G=-1\times 96500\times 1.02$ ;

$\Delta G=-98430$ .