SECTION - A Consider the following standard electrode potential values: {\Sn}_{( {\aq})}^{2+}+2 {\e}^{-} \to {\Sn}_{( { s})} {\E}^0 =-0.14 {\V} {Fe}^{3+}{ }_{({aq})}+{e}^{-} \\to {Fe}^{2+}{}_{({aq})} {E}^0 =+0.77 {V} What is the cell reaction and potential for the spontaneous reaction that occurs?

Correct Answer is : 2Fe3+(aq)+Sn(s)→2Fe2+(aq) +Sn2+(aq)E°=+0.94V

{2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})} \\to2 {Fe}^{3+}{ }_{({aq})} +{Sn}_{({s})} {E}^0=-0.91V

2{Fe^{3+}}_{(aq)}+Sn_(s)\to{2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})}E^\circ=+0.94V

{2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})} \\to2 {Fe}^{3+}{ }_{({aq})} +{Sn}_{({s})} {E}^0=+0.91V

2{Fe^{3+}}_{(aq)}+Sn_(s)\to{2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})}E^\circ=+1.68V

CBSE Class 12 Chemistry 2023 Delhi Set 3 Solved Paper

Question : 1 of 13

Marks: +1, -0

SECTION - A

Consider the following standard electrode potential values:

{\Sn}_{( {\aq})}^{2+}+2 {\e}^{-} → {\Sn}_{( {\ s})} {\E}^0

=-0.14 {\V}

{Fe}^{3+}{ }_{({aq})}+{e}^{-} \→ {Fe}^{2+}{}_{({aq})} {E}^0

=+0.77 {V}

What is the cell reaction and potential for the spontaneous reaction that occurs?

${2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})} \→2 {Fe}^{3+}{ }_{({aq})}$ $+{Sn}_{({s})} {E}^0=-0.91V$
$2{Fe^{3+}}_{(aq)}+Sn_(s)→{2Fe^{2+}}_{(aq)}$ $+{{Sn}^{2+}}_{({aq})}E°=+0.94V$
${2Fe^{2+}}_{(aq)} +{{Sn}^{2+}}_{({aq})} \→2 {Fe}^{3+}{ }_{({aq})}$ $+{Sn}_{({s})} {E}^0=+0.91V$
$2{Fe^{3+}}_{(aq)}+Sn_(s)→{2Fe^{2+}}_{(aq)}$ $+{{Sn}^{2+}}_{({aq})}E°=+1.68V$

Solution:

{E}°={E}_{{C}}-{E}_{{a}}

=0.77-(-0.14)=+0.94 {V}

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