The standard reduction potential of the reaction- H2O-e-1-2H2-OH at 298K is-

The correct option is B E^o= RT/Fln[P_H_2]^1/2[OH^ ] E _ cell =0 at eq ^ m 0= E _ cell ^ o + RT F ln[ P _ H _ 2 ]^ 1 / 2 [ OH ^ ] ...

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Electrolytic Cell

The standard ...

Question

The standard reduction potential of the reaction, $H_{2} O + e^{-} \to \frac{1}{2} H_{2} + O H$ at $298$ K is:

E^{o} = \frac{R T}{F} l n K_{w}

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E^{o} = - \frac{R T}{F} l n [P_{H_{2}}]^{1 / 2} [O H^{-}]

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E^{o} = - \frac{R T}{F} l n \frac{[P_{H_{2}}]^{1 / 2}}{[H^{+}]}

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E^{o} = - \frac{R T}{F} l n K_{w}

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Z n^{+ 2} + 2 e^{-} ⇌ Z n; E^{o} = - 0.76 V

A g^{+} + e^{-} ⇌ A g; E^{o} = + 0.80 V

E = E^{o} - \frac{R T}{n F} l n Q

Q = K_{c}

298 K

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{o} = - 0.28 V

M g^{2 +} (a q) + 2 e^{-} \to M g (s); E^{o} = - 2.37 V

E^{o}

Z n \to {Z n}^{2 +} + 2 e^{-}; E^{o} = + 0.76 V

F e \to {F e}^{2 +} + 2 e^{-}; E^{o} = + 0.41 V

{F e}^{2 +} + Z n \to {Z n}^{2 +} + F e

E^{o}

Z n \to Z n^{2 +} + 2 e^{-}; E^{o} = - 0.76 V

F e^{2 +} + 2 e^{-} \to F e; E^{o} = + 0.41 V

F e^{2 +} + Z n \to Z n^{2 +} + F e

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