What is the reaction occurring at the anode in a $CH_4 - O_2$ fuel cell?
- A$2O_2 + 8H^{+} + 8e^{-} \rightarrow 4H_2O$
- B$CH_4 + 2H_2O \rightarrow CO_2 + 8H^{+} + 8e^{-}$
- C$CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$
- D$2H^{+} + 2e^{-} \rightarrow H_2$
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View SolutionThe Gibbs energy for the decomposition of $Al_2O_3$ at $500^oC$ is as follows:
$\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$
$\Delta_rG = +960 \ kJ \ mol^{-1}$
The potential difference needed for the electrolytic reduction of aluminium oxide $(Al_2O_3)$ at $500^oC$ is at least ........ $V$.
$\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$
$\Delta_rG = +960 \ kJ \ mol^{-1}$
The potential difference needed for the electrolytic reduction of aluminium oxide $(Al_2O_3)$ at $500^oC$ is at least ........ $V$.
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