The standard electrode potential for the Daniell cell is $1.1 \ V$. What will be the value of standard Gibbs energy for the reaction?
$Zn_{(s)} + Cu_{(aq)}^{2+} \rightarrow Zn_{(aq)}^{2+} + Cu_{(s)}$
$(1 \ F = 96487 \ C \ mol^{-1})$
$Zn_{(s)} + Cu_{(aq)}^{2+} \rightarrow Zn_{(aq)}^{2+} + Cu_{(s)}$
$(1 \ F = 96487 \ C \ mol^{-1})$
- A$-106.14 \ kJ \ mol^{-1}$
- B$212.27 \ kJ \ mol^{-1}$
- C$-212.27 \ kJ \ mol^{-1}$
- D$106.14 \ kJ \ mol^{-1}$
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