Duration: 5:49

853 views

18

Given bol:w are the half-cell reactions :
\[
\mathrm{Mn}^{2+}+2 e^{-} \longrightarrow \mathrm{Mn} ; E^{\circ}=-1.18 \mathrm{~V}
\]
\[
2\left(\mathrm{Mn}^{3+}+e^{-} \longrightarrow \mathrm{Mn}^{2+}\right) ; \quad E^{0}=+1.51 \mathrm{~V}
\]
The \( E^{\circ} \) for \( 3 \mathrm{Mn}^{2+} \longrightarrow \mathrm{Mn}+2 \mathrm{Mn}^{3+} \) will be :
(A) \( -2.69 \mathrm{~V} \); the reaction will not occur
(B) \( 2.69 \mathrm{~V} \); the reaction will occur
(C) \( -0.33 \mathrm{~V} \); the reaction will not occur
(D) \( -0.33 \mathrm{~V} \); the reaction will occur
📲PW App Link - https://bit.ly/YTAI_PWAP
🌐PW Website - https://www.pw.live