Respuesta :
Answer : The correct option is, (C) 6
Explanation :
Oxidation-reduction reaction : It is a reaction in which oxidation and reduction reaction occur simultaneously.
Oxidation reaction : It is the reaction in which a substance looses its electrons. In this oxidation state increases.
Reduction reaction : It is the reaction in which a substance gains electrons. In this oxidation state decreases.
The given unbalanced chemical reaction is,
[tex]Fe(s)+I^-(aq)\rightarrow I_2(s)+Fe^{3+}(aq)[/tex]
Half reactions of oxidation and reduction are :
Oxidation : [tex]Fe(s)\rightarrow Fe^{3+}+3e^-[/tex] ......(1)
Reduction : [tex]2I^-(aq)+2e^-\rightarrow I_2[/tex] .......(2)
In order to balance the electrons, we multiply equation 1 by 2 and equation 2 by 3, we get:
Oxidation : [tex]2Fe(s)\rightarrow 2Fe^{3+}+6e^-[/tex] ......(1)
Reduction : [tex]6I^-(aq)+6e^-\rightarrow 3I_2[/tex] .......(2)
The overall balanced chemical reaction will be:
[tex]2Fe(s)+6I^-(aq)\rightarrow 3I_2(s)+2Fe^{3+}(aq)[/tex]
From this reaction we conclude that the electrons are getting transferred from iron to iodine and the number of electrons transferred are 6 electrons.
Hence, the correct option is, (C) 6
