The standard cell potential for Zn mid Zn^{2+ | vedclass

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Question

(A) The cell reaction is: $Zn_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$According to the Nernst equation:$E_{cell} = E^{\circ}_

Vedclass · Accepted Answer

$37.3$

Vedclass · Answer

(A) The cell reaction is: $Zn_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$According to the Nernst equation:$E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}$When the cell is completely discharged,$E_{cell} = 0$ and $n = 2$.Substituting the values:$0 = 1.10 - \frac{0.0591}{2} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}$$1.10 = \frac{0.0591}{2} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}$$\log \frac{[Zn^{2+}]}{[Cu^{2+}]} = \frac{1.10 	imes 2}{0.0591} = \frac{2.20}{0.0591} \approx 37.225$Thus,the value is closest to $37.3$.

The standard cell potential for $Zn \mid Zn^{2+} \parallel Cu^{2+} \mid Cu$ is $1.10 \ V$. When the cell is completely discharged,$\log ([Zn^{2+}] / [Cu^{2+}])$ is closest to $.....$

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