Question

Identify the species that is oxidized and the species that is reduced in the reaction. White out half reactions to show how many electrons are gained or lost by each species.
Zn(s)+2H+(aq)->Zn2+(aq)+H2(g)

Answer 1

$Zn(s)+2H^+(aq)->Zn^{2+}(aq)+H_2(g)$

Oxidized species --- Zn(s)

Reduced species ---H⁺(aq)

Half Reactions

$Zn(s)->Zn^{2+}(aq)+2.e^{-}$

$2H^+(aq)+2.e^-->H_2(g)$