Question

For the electrochemical cell:

\[\ce{M | M+ || X- | X}\]; 

\[\ce{E^{\circ}_{{M^{+}/{M}}}}\] = 0.44 V,

\[\ce{E^{\circ}_{X/X^-}}\] = 0.33 V

Which of the following is TRUE for this data?

For the electrochemical cell \[\ce{M | M+ || X- | X}\]; \[\ce{E^{\circ}_{{M^{+}/{M}}}}\] = 0.44 V, \[\ce{E^{\circ}_{X/X^-}}\] = 0.33 V. From this data, one can deduce that:

विकल्प

• \[\ce{E^{\circ}_{cell}}\] = −0.77V

• \[\ce{E^{\circ}_{cell}}\] = 0.77V

• \[\ce{M+ + X- -> M + X}\] is a spontaneous reaction.

• \[\ce{M + X -> M+ + X-}\] is a spontaneous reaction.

Answer 1

\[\ce{M+ + X- -> M + X}\] is a spontaneous reaction.

Explanation:

Cell reaction: \[\ce{M + X -> M^+ + X^-}\]

The anode is M, and the cathode is X.

\[\ce{E{^{\circ}_{cell}} = E{^{\circ}_{cathode}} - E{^{\circ}_{anode}}}\]

= 0.33 − 0.44

= −0.11 V

Since \[\ce{E{^{\circ}_{cell}}}\] is negative, the cell reaction is non-spontaneous.

∴ The reverse reaction, \[\ce{M^+ + X^- -> M + X}\] is the spontaneous reaction.