Oxidation and reduction process involves the transaction of electrons. Loss of electrons is oxid....
0Oxidation and reduction process involves the transaction of electrons. Loss of electrons is oxidation and the gain of electrons is reduction. It is thus obvious that in a redox reaction, the oxidant is reduced by accepting the electrons
\( \mathrm{P} \)
and the reductant is oxidized by losing electrons. The reactions in which a species disproportionates into two oxidation states (lower and higher) are called disproportionation reactions. In electrochemical cells, redox reaction is involved, i.e., oxidation takes place at anode and reduction at cathode.
Which of the following reactions(s) is/are not correctly indicated?
Oxidant + Reductant
(1) \( \mathrm{HNO}_{3}+\mathrm{Cu} \rightarrow \mathrm{Cu}^{2+}+\mathrm{NO}_{2} \)
(2) \( 2 \mathrm{Zn}+\mathrm{O}_{2} \rightarrow \mathrm{ZnO} \)
(3) \( \mathrm{Cl}_{2}+2 \mathrm{Br}^{-} \rightarrow 2 \mathrm{Cl}^{-}+\mathrm{Br}_{2} \)
(4) \( 4 \mathrm{Cl}_{2}+\mathrm{CH}_{4} \rightarrow \mathrm{CCl}_{4}+4 \mathrm{HCl} \)
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