• # question_answer Check the feasibility of the following redox reaction with the help of electrochemical series $Ni(s)+2A{{g}^{+}}(aq)\,\xrightarrow{\,}N{{i}^{2+}}(aq)+2Ag(s)$

The E° value of $N{{i}^{2+}}/Ni$ is ? 0.25V while that of $A{{g}^{+}}/Ag$ is +0.80 V. This means that nickel is placed below silver in the series and can easily reduce $A{{g}^{+}}$ ions to silver by releasing electrons. The redox reaction is therefore, feasible.