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Oxidising and Reducing Nature

Which of the ...

Question

Which of the following statement is true regarding the given standard reduction potential?
Given:
$A g^{+} + e^{-} \to A g; E^{0} = + 0.8 V N i^{2 +} + 2 e^{-} \to N i; E^{0} = - 0.25 V .$

A g^{+}

can act as an oxidising agent while

N i

can act as a reducing agent

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N i^{2 +}

can act as an oxidising agent while

A g

can act as a reducing agent

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A g

can displace

N i

from

N i S O_{4}

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A g

is highly reactive as compared to

N i

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Solution

The correct option is A $A g^{+}$ can act as an oxidising agent while $N i$ can act as a reducing agent
In the given problem,
$E_{A g + / A g}^{0} = + 0.8 V$
$E_{N i^{2 +} / N i}^{0} = - 0.25 V$
Here, $E_{A g^{+} / A g}^{0} > E_{N i^{2 +} / N i}^{0}$
So, $A g^{+}$ acts as an oxidising agent and $N i^{2 +}$ acts as a reducing agent.
Metals which have high reduction potential will have more tendency to get reduce and exist in metal form. Hence, they are unreactive metals.

Metals which have less reduction potential will have more tenducy to get oxidise and exist in ionic forms. Hence, they are highly reactive metals.

Since, $N i$ is the reactive metal, it can displace $A g$ from $A g N O_{3}$

So, correct answer is option A.

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