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Two metals 'A' and 'B' have $\mathrm{E}_{\text {red }}^{\circ}$ value equal to 0.36 V and 1.23 V . What will be the correct cell equation?
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The correct answer is:
$\mathrm{A}+\mathrm{B}^{2+} \longrightarrow \mathrm{A}^{2+}+\mathrm{B}$
From $E_{\text {red }}^{\circ}$. values, it is clear that $A$ is more electropositive than $B$ (as it has lesser $E^{\circ}{ }_{\text {red }}$ ), hence it can replace $B$ from its salt solution and act as anode in galvanic cell. Hence, correct cell equation will be:
$A+B^{2+} \longrightarrow A^{2+}+B$
$A+B^{2+} \longrightarrow A^{2+}+B$
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