In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced:
(its multiple choice)
Number 1:
Br2(g)+2KI(aq)→2KBr(aq)+I2(s)
I− (in KI) loses electrons and is oxidized. Br2 gains electrons and is reduced. | ||||||||
Br2 gains electrons and is oxidized. I− (in KI) loses electrons and is reduced. | ||||||||
I− (in KI) gains electrons and is oxidized. Br2 loses electrons and is reduced. | ||||||||
Br2 loses electrons and is oxidized. I− (in KI) gains electrons and is reduced. Number 2: Sn(s)+Cu2+(aq)→Sn2+(aq)+Cu(s)
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Br2(g)+2KI(aq)→2KBr(aq)+I2(s)
Bromine gains electron and the oxidation number decreases from 0 to -1 (Oxidation number of Br in KBr is -1).Iodine loses electron and the oxidation number increases from -1(Oxidation number of iodine in KI is -1) to 0. Thus, Bromine is getting reduced and Iodine is getting oxidized
Sn(s)+Cu2+(aq)→Sn2+(aq)+Cu(s)
Tin (Sn) loses two electron and the oxidation number increases from 0 to +2 .Copper(Cu) gains two electron and the oxidation number decreases from +2 to 0. Thus, Tin (Sn) is getting oxidized and Copper is getting reduced.
Fe(s)+CuSO4(aq)→FeSO4(aq)+Cu(s)
Fe loses two electron and the oxidation number increases from 0 to +2 (Oxidation number of Fe in FeSO4 is +2) .Copper(Cu) gains two electron and the oxidation number decreases from +2(Oxidation number of Cu in CuSO4) to 0. Thus, Fe is getting oxidized and Copper is getting reduced.
In each of the following reactions, identify the reactant that is oxidized and the reactant that...
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