Identify the reactant that is oxidized (loses electrons) in this reaction

Question

2HCl_(aq) + Zn_(s)  --->   H_2(g)  +  Zn²⁺_(aq) + 2 Cl^–_(aq)

Answer 1

It's always easiest to look at the oxidation numbers of each element on each side of the equation and see which gains and which loses electrons.

2 H - Cl(aq) + Zn(s) ===> H2(g) + Zn2+(aq) + 2 Cl-(aq)

..+1...-1..............0..................0............+2....................-1.............Oxidation numbers

So, H went from +1 to zero so it gained an electron so it was reduced

Zn went from zero to +2, so it lost electrons and was oxidized.

So, answer is Zn(s)