All the energy released from the reaction X- Y- rG- - -193 kJ mol-1 is used for oxidising M- as M- M3- - 2e- E- - -0-25 V- Under standard conditions- the number of moles of M- oxidised when one mole of X is converted to Y is- F - 96500 C mole-1

#160; _rG^∘ = 193 kJ/ mol #160; M^+→ M^3+ + 2e^ G^∘ for above reaction is: G^∘ = nFE^∘ #160; #160; #160; #160; #160; ...

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Gibbs Free Energy & Spontaneity

All the energ...

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All the energy released from the reaction $X \to Y, △_{r} G^{\circ} = - 193 k J m o l^{- 1}$ is used for oxidising $M^{+}$ as $M^{+} \to M^{3 +} + 2 e^{-}, E^{\circ} = - 0.25 V$ . Under standard conditions, the number of moles of $M^{+}$ oxidised when one mole of $X$ is converted to $Y$ is: $(F = 96500 C m o l e^{- 1})$

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X \to Y; Δ G^{\circ} = - 193 {kJ mol}^{- 1}

M^{+}

M^{+} \to M^{3 +} + 2 e^{-}; E^{\circ} = - 0.25 V

M^{+}

[F = 96500 C m o l^{- 1}]

X \to Y, Δ_{r} G^{\circ} = - 193 k J . m o l^{- 1}

M^{+}

M^{+} \to M^{3 +} + 2 e^{-}, E^{\circ} = - 0.25 V .

M^{+}

[F = 96500 C m o l^{- 1}]

X \to Y, Δ_{r} G^{0} = - 193 {kJ mol}^{- 1}

M^{+} \to M^{3 +} + 2 e^{-}, E^{0} = - 0.25 V

M^{+}

X

Y

F = 96500 {C mol}^{- 1}

M^{x +} + M n O_{4}^{-} \to M O_{3}^{-} + M n^{2 +}

M n O_{4}^{-}

M^{x +}

M^{x +} + M n O_{4}^{-} \to M O_{3}^{-} + M n^{2 +} + \frac{1}{2} O_{2}

M n O_{4}^{-}

M^{x +}

M O_{3}^{-}

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