A cell is constructed using Ag+/Ag and Au3+ /Au electrodes. If E0 values of Ag and Au electrodes are 0.80 V and 1.40 V. Then the cell reaction is

Ag/Ag+//Au3+/Au3Ag+Au3+→3Ag++Au

A cell is constructed using Ag+/Ag and Au3+ /Au electrodes. If E0 values of Ag and Au electrodes are 0.80 V and 1.40 V. Then the cell reaction is

Ag/Ag+//Au3+/Au3Ag+Au3+→3Ag++Au

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A cell is constructed using Ag⁺/Ag and Au³⁺/Au electrodes. If E⁰ values of Ag and Au electrodes are 0.80 V and 1.40 V. Then the cell reaction is

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3Ag + Au³⁺ → 3Ag⁺ + Au

Au + 3Ag⁺ → Au³⁺ + 3Ag

Ag + Au³⁺ → AgAu

2Ag + Au²⁺ → 2Ag⁺ + Au

answer is A.

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$\begin{array}{l} Ag / {Ag}^{+} / / {Au}^{3 +} / Au \\ 3 Ag + {Au}^{3 +} \to 3 {Ag}^{+} + Au \end{array}$

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A cell is constructed using Ag+/Ag and Au3+ /Au electrodes. If E0 values of Ag and Au electrodes are 0.80 V and 1.40 V. Then the cell reaction is

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A cell is constructed using Ag⁺/Ag and Au³⁺/Au electrodes. If E⁰ values of Ag and Au electrodes are 0.80 V and 1.40 V. Then the cell reaction is