Question

Which one is correct about a hypothetical electrochemical cell shown below?
$\underset{A}{\ominus }|A^{+}\left(XM\right)||B^{+}\left(YM\right)|\underset{B}{\oplus }{E}_{cell}=+0.20V$

• A. The cell reaction cannot be predicted
• B. $A+B^{+}\to A^{+}+B$
• C. $A^{+}+B\to A+B^{+}$
• D. $A^{+}+e\to A;B^{+}+e\to B$

Answer 1

Answer: (B)

$A+B^{+}\to A^{+}+B$

For Cell,
$A|A^{+}\left(XM\right)||B^{+}\left(YM\right)|B{E}_{cell}=+0.20V$
reaction of cell
At anode (oxidation): $A\to A^{+}+e$,
At cathode (reduction): $B^{+}+e\to B$
Net Reaction: $A+B^{+}\to A^{+}+B;E_{cell}=+ve$
As emf of cell is positive so reaction is spontaneous forward.