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# Calculation: $\Delta {G}^{°}$ of a Cell Reaction

CHEM-4SZZTN

Calculate $\Delta {G}^{°}$ (in kJ) for the reaction:

$$2AgCl (aq) + Zn (s) \xrightarrow [ ]{ } 2Ag (s) + Zn{Cl}_{2} (aq)$$

$\Delta {G}^{°} = -nF{E}^{°}$
Faraday's constant, $F = 96485\ \frac{C}{mol\ {e}^{-}}$
Half-reaction ${E}^{°}$
${Ag}^{2+} + {e}^{-} \xrightarrow [ ]{ } {Ag}^{+}$ $1.99\ V$
${Ag}^{+} + { e }^{ - } \xrightarrow [ ]{ } Ag$ $0.80\ V$
${Zn}^{2+} + 2{ e }^{ - } \xrightarrow [ ]{ } Zn$ $-0.76\ V$