Question

The following reaction is feasible or not feasible and why?

\[\ce{I2 + 2NaCl -> 2NaI + Cl2}\]

Answer 1

The given reaction is:

\[\ce{I2 + 2NaCl -> 2NaI + Cl2}\]

Reduction reaction: \[\ce{I2 + 2e- -> 2I-}\]

Oxidation reaction: \[\ce{2Cl- -> Cl2 + 2e-}\]

Standard electrode potentials (E°) are:

\[\ce{E^{\circ}_{I_2/I^-}}\] = +0.54 V

\[\ce{E^{\circ}_{Cl_2/Cl^-}}\] = +1.36 V

Cell potential:

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

= 0.54 − 1.36

= −0.82 V

Since \[\ce{E^{\circ}_{cell}}\] is negative, the reaction is not feasible under standard conditions.