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(A) reaction is spontaneous if the standard cell potential $E^\circ_{cell}$ is positive. According to the Electrochemical Series,a metal with a lower

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$Cu_{(s)} + 2AgNO_{3(aq)} 	o Cu(NO_3)_{2(aq)} + 2Ag_{(s)}$

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(A) reaction is spontaneous if the standard cell potential $E^\circ_{cell}$ is positive. According to the Electrochemical Series,a metal with a lower (more negative) standard reduction potential can displace a metal with a higher (more positive) standard reduction potential from its salt solution. For option $A$: $Cu_{(s)} + 2Ag^+_{(aq)} 	o Cu^{2+}_{(aq)} + 2Ag_{(s)}$. Here,$E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} = E^\circ_{Ag^+/Ag} - E^\circ_{Cu^{2+}/Cu} = 0.80 \ V - 0.34 \ V = +0.46 \ V$. Since $E^\circ_{cell} > 0$,the reaction is spontaneous. For options $B, C,$ and $D$,the metal being oxidized has a higher reduction potential than the metal being reduced,resulting in a negative $E^\circ_{cell}$,making them non-spontaneous.

Which among the following reactions will take place spontaneously?

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