Chapter 17, Problem 61QAP

Interpretation Introduction

Interpretation:

The standard reduction potential at 25°C for the half-reaction needs to be identified.

${\text{Ag}}_{\text{2}}{\text{CrO}}_{\text{4}}\left(\text{s}\right){\text{ + 2e}}^{\text{-}}\to \text{2Ag}\left(\text{s}\right){\text{ + CrO}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right)$

Concept introduction:

A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction. The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, it gets oxidized.

An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s.

Spontaneity of a reaction is dependent on the free energy sign that is $\Delta G^o$. It should be negative for a reaction to be spontaneous.

Since,

$\Delta G=-nF{E}^o$

Here, n = number of electrons involved in reaction and F is Faraday’s constant.

If the value of E° for a reaction is positive, then the reaction occurs spontaneous.