Given below are half-cell reactions: \[ \begin{array}{l} \mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5...
0Given below are half-cell reactions:
\[
\begin{array}{l}
\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \longrightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \\
\mathrm{E}_{\mathrm{Mn}^{2+} / \mathrm{MnO}_{4}^{-}}^{\circ}=-1.510 \mathrm{~V} \\
\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 e^{-} \longrightarrow \mathrm{H}_{2} \mathrm{O} ; E_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\circ}=+1.223 \mathrm{~V}
\end{array}
\]
- Will the permanganate ion, \( \mathrm{MnO}_{4}^{-} \)liberate \( \mathrm{O}_{2} \) from water in the presence of an acid?
(a) Yes, because \( E_{\text {cell }}^{\circ}=+0.287 \mathrm{~V} \)
(b) No, because \( E_{\text {cell }}^{\circ}=-0.287 \mathrm{~V} \)
(c) Yes, because \( E_{\text {cell }}^{\circ}=+2.733 \mathrm{~V} \)
(d) No, because \( E_{\text {cell }}^{\circ}=-2.733 \mathrm{~V} \)
š²PW App Link - https://bit.ly/YTAI_PWAP
šPW Website - https://www.pw.live