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

For the reaction M^+→ M^3++2e^ , , the standard Gibbs free energy change is Δ #160; G^0 = nFE^0 = 2 × 96500 × ( 0.25) = 48250 J/mol = 48.25 kJ ...

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Gibb's Energy and Nernst Equation

All the energ...

Question

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

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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^{0} = - 193 {kJ mol}^{- 1}

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

M^{+}

X

Y

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

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

M^{+}

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

M^{+}

X

Y

(F = 96500 C m o l e^{- 1})

F e

O_{2}

F e O

F e_{2} O_{3}

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

M n O_{4}^{-}

M^{x +}

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