Question

Consider the following redox reaction. 2MnO$_4^-$ (aq) + 2H$_2$O(l) + 6H$^+$ (aq) $\longrightarrow$ 2Mn$^{2+}$ (aq) + 5H$_2$O$_2$(l) In the given redox reaction, MnO$_4^-$ is the oxidizing agent and H$_2$O is the reducing agent. The balanced chemical equations for the two half-reactions are 2H$_2$O(l) $\longrightarrow$ H$_2$O$_2$(l) + 2H$^+$ (aq) + 2e$^-$ E$^o_{red, H_2O_2}$ = 1.776 V MnO$_4^-$ (aq) + 8H$^+$ (aq) + 5e$^-$ $\longrightarrow$ Mn$^{2+}$ (aq) + 4H$_2$O(l) E$^o_{red, MnO_4^-}$ = 1.507 V 1st attempt Calculate $\Delta G^o$: ____ kJ

          Consider the following redox reaction.
2MnO$_4^-$ (aq) + 2H$_2$O(l) + 6H$^+$ (aq) $\longrightarrow$ 2Mn$^{2+}$ (aq) + 5H$_2$O$_2$(l)
In the given redox reaction, MnO$_4^-$ is the oxidizing agent and H$_2$O is the reducing agent.
The balanced chemical equations for the two half-reactions are
2H$_2$O(l) $\longrightarrow$ H$_2$O$_2$(l) + 2H$^+$ (aq) + 2e$^-$  E$^o_{red, H_2O_2}$ = 1.776 V
MnO$_4^-$ (aq) + 8H$^+$ (aq) + 5e$^-$ $\longrightarrow$ Mn$^{2+}$ (aq) + 4H$_2$O(l)  E$^o_{red, MnO_4^-}$ = 1.507 V
1st attempt
Calculate $\Delta G^o$: ____ kJ

Consider the following redox reaction.
2MnO4^- (aq) + 2H2O(l) + 6H^+ (aq) ⟶ 2Mn^2+ (aq) + 5H2O2(l)
In the given redox reaction, MnO4^- is the oxidizing agent and H2O is the reducing agent.
The balanced chemical equations for the two half-reactions are
2H2O(l) ⟶ H2O2(l) + 2H^+ (aq) + 2e^- E^ored, H2O2 = 1.776 V
MnO4^- (aq) + 8H^+ (aq) + 5e^- ⟶ Mn^2+ (aq) + 4H2O(l) E^ored, MnO4^- = 1.507 V
1st attempt
Calculate Δ G^o: kJ

Added by William C.

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