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Question
The following reaction is feasible or not feasible and why?
\[\ce{I2 + 2NaCl -> 2NaI + Cl2}\]
Long Answer
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Solution
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.
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Chapter 7: p-Block Elements - SHORT ANSWER TYPE QUESTIONS [Page 448]
