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Standard Electrode Potentials

The standard ...

Question

The standard reduction potential of $Z n^{2 +} / Z n$ system is $- 0.76 V$ . This means :

A

Z n O

is reduced to

Z n

by

H_{2}

.

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B

Z n

is generally the cathode in an electrochemical cell.

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C

Z n

is generally the anode in an electrochemical cell.

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D

None of the above.

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Solution

The correct option is D $Z n$ is generally the anode in an electrochemical cell.
The standard reduction potential of zinc is negative $(- 0.76 V)$ . Zn has a high tendency to lose electrons and hence, it forms an anode in an electrochemical cell.

The reaction at anode is as follows:
$Z n \to Z n^{2 +} + 2 e^{-}$

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Similar questions

In an electrochemical cell represented as,

Zn | Zn²⁺₍c₁₎ || Cu²⁺₍c₂₎| Cu

So in this cell,

a.Zn is oxidized

b.Zn is reduced

c.Cu is oxidized

d.Cu is reduced

Q. The standard reduction potential

E^{o}

for half reactions are,

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

The emf of the cell reaction;

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

Q. In the following electrochemical cell :

Z n | Z n^{2 +} | | H^{\oplus} | (H_{2}) P t

E_{c e l l} =_{c e l l}^{⊖}

. This will be when :

Q. The standard reduction potential

E^{o}

for the half reactions are as

Z n ⟶ {Z n}^{2 +} + 2 e^{-}

E^{o} = + 0.76 V

F e ⟶ {F e}^{2 +} + 2 e^{-}

E^{o} = + 0.41 V

The emf for cell reaction,

{F e}^{2 +} + Z n ⟶ {Z n}^{2 +} + F e

At 298 K, the standard reduction potentials for the following half-reactions are given. Which acts as an anode with others in an electrochemical cell?

$Z n^{+ 2} (a q) + 2 e^{-} \to Z n (s),$ -0.762 V

$C r^{+ 3} (a q) + 3 e^{-} \to C r (s),$ -0.740 V

$2 H^{+} (a q) + 2 e^{-} \to H_{2} (g),$ 0.000 V

$F e^{+ 3} (a q) + e^{-} \to F e^{2 +} (a q),$ +0.762 V

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