Upon dipping a copper rod into an aqueous sol | vedclass

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(D) The correct option is $D$. When a copper rod is dipped into an aqueous solution of $AgNO_{3}$,a displacement reaction occurs because copper is mor

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$AgNO_{3}$

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(D) The correct option is $D$. When a copper rod is dipped into an aqueous solution of $AgNO_{3}$,a displacement reaction occurs because copper is more reactive than silver.$Cu_{(s)} + 2AgNO_{3(aq)} \longrightarrow Cu(NO_{3})_{2(aq)} + 2Ag_{(s)}$In this reaction,$Cu$ is oxidized to $Cu^{2+}$ ions,which impart a blue color to the solution.The half-cell reactions are:$Cu_{(s)} \longrightarrow Cu^{2+}_{(aq)} + 2e^{-}; E^{\circ} = -0.34 \, V$$Ag^{+}_{(aq)} + e^{-} \longrightarrow Ag_{(s)}; E^{\circ} = 0.80 \, V$The overall cell potential is positive,indicating the reaction is spontaneous.

List-$I$ (Applications)	List-$II$ (Batteries/Cell)
$A$. Transistors	$I$. Anode $- Zn/Hg$; Cathode $- HgO + C$
$B$. Hearing aids	$II$. Hydrogen fuel cell
$C$. Inverters	$III$. Anode $- Zn$; Cathode $- Carbon$
$D$. Apollo space ship	$IV$. Anode $- Pb$; Cathode $- PbO_2$

Upon dipping a copper rod into an aqueous solution of the salt,the solution that turns blue is

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The Gibbs energy change (in $J$) for the given reaction at $[Cu^{2+}] = [Sn^{2+}] = 1 \, M$ and $298 \, K$ is:
$Cu_{(s)} + Sn^{2+}_{(aq)} \rightarrow Cu^{2+}_{(aq)} + Sn_{(s)}$
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