Question

A galvanic cell consists of a Ni2+/ Ni half-cell and a standard hydrogen electrode.

If the Ni2+/ Ni half-cell standard cell functions as the anode, and the standard cell potential is 0.26 V, what is the standard reduction potential for the Ni2+/Ni half-cell?
A) - 0.26 V
B) - 0.13 V
C) + 0.13 V
D) + 0.26 V

Answer 1

Answer:

A) - 0.26 V

Explanation:

Here Ni undergoes oxidation by loss of electrons, thus act as anode. Standard hydrogen electrode undergoes reduction by gain of electrons and thus act as cathode.

$E^0=E^0_{cathode}- E^0_{anode}$

Where both $E^0$ are standard reduction potentials.

Given that:- $E^0=0.26\ V$

Also, $E^0_{[H^{+}/H_2]}=0\ V$

So,

$E^0=E^0_{[H^{+}/H_2]}-E^0_{[Ni^{2+}/Ni]}$

$0.26\ V=0\ V- E^0_{[Ni^{2+}/Ni]}$

$E^0_{[Ni^{2+}/Ni]}=-0.26\ V$

Answer 2

The standard reduction potential for the Ni2+/Ni half-cell is - 0.26 V.

What is standard hydrogen electrode?

The standard hydrogen electrode is a reference electrode that was arbitrarily assigned an electrode potential of 0.00V. We know that metals that are above hydrogen in the electrochemical series will always have a negative electrode potential.

As such, the standard reduction potential for the Ni2+/Ni half-cell is - 0.26 V.

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