Question

A hypothetical electrochemical cell is shown below :- $\overset{T}{A}|A+(xM)||B^+(yM)|\overset{\oplus}{B}$ The emf measured is +0.20V. The cell reaction is:

• A. $A+B^+ \rightarrow A^+ \, +B$
• B. $A^++B \rightarrow A \, +B^+$
• C. $A^+ \, +e^- \rightarrow A,B^+\, +e^- \rightarrow B$
• D. the cell reaction cannot be predicted

Answer 1

Answer: (A)

$A+B^+ \rightarrow A^+ \, +B$

Answer 2

$A / A ^{+}( xM )|| B ^{+}( yM ) \overline{ B }$
$E _{\text {cell }}=+0.20 V \quad \therefore \Delta G =- Ve$

Therefore given cell reaction is spontaneous

At $A \rightarrow A ^{+}+ e ^{-}$

At Cathode $\underline{ B ^{+}+ e ^{-} \rightarrow B }$

Cell reaction $A + B ^{+} \rightarrow A ^{+}+ B$