Q74 / 160 · JIPMER 2004 · Chemistry
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?
- Correct answerA$\mathrm{A}+\mathrm{B}^{2+} \longrightarrow \mathrm{A}^{2+}+\mathrm{B}$
- B$\mathrm{A}^{2+}+\mathrm{B} \longrightarrow \mathrm{A}+\mathrm{B}^{2+}$
- CBoth (1) and (2)
- DNone of the above
Solution
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:
$A+B^{2+} \longrightarrow A^{2+}+B$
Hence, the correct answer is option: 'A'.