The standard potential of the cell in the following reaction is _____. $Cd_{(s)} + Cu^{2+}_{(1M)} \longrightarrow Cd^{2+}_{(1M)} + Cu_{(s)}$ ($E^\circ_{Cd} = -0.403V$, $E^\circ_{Cu} = 0.334V$) (a) –0.737 V (b) 0.737 V (c) –0.069 V (d) 0.069 V

The standard potential of the cell in the following reaction is ___. Cd(s) + Cu²⁺(1M) longrightarrow Cd²⁺(1M)

Question 95 of 111

Cd_{(s)} + Cu^{2+}_{(1M)} \longrightarrow Cd^{2+}_{(1M)} + Cu_{(s)}

(a) –0.737 V

(b) 0.737 V

(d) 0.069 V

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Cd is oxidised (anode) and Cu²⁺ is reduced (cathode); subtracting their standard potentials gives +0.737 V.

In the reaction $Cd(s) + Cu^{2+}(1M) \rightarrow Cd^{2+}(1M) + Cu(s)$ , cadmium is oxidised (anode) and copper(II) ion is reduced (cathode). The standard cell potential is: …

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Q.The standard potential of the cell in the following reaction is _____. $Cd_{(s)} + Cu^{2+}_{(1M)} \longrightarrow Cd^{2+}_{(1M)} + Cu_{(s)}$ ( $E^\circ_{Cd} = -0.403V$ , $E^\circ_{Cu} = 0.334V$ )

Concept understanding — Electrochemical Cells

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