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

Br2(aq)+2I-(aq)->2Br-(aq)+I2(aq)

Name one compound containing H+ ions and another containing I- ions, which would be suitable for these reactions.

Ezplain why zinc is said to be oxidised in its reaction.

Complete the half equation to show the oxidising action of bromine.
_I- ->I2+____

Answered above.

A compound containing H+ ions that would be suitable for the reaction is hydrochloric acid (HCl). In hydrochloric acid, H+ ions are produced when the acid dissociates in water:

HCl(aq) -> H+(aq) + Cl-(aq)

A compound containing I- ions that would be suitable for the reaction is potassium iodide (KI). When potassium iodide dissolves in water, it dissociates into K+ and I- ions:

KI(aq) -> K+(aq) + I-(aq)

Now, let's explain why zinc is considered to be oxidized in its reaction. In the given reaction Zn(s) + 2H+(aq) -> Zn2+(aq) + H2(g), the oxidation state of zinc changes from 0 in the reactant (Zn(s)) to +2 in the product (Zn2+(aq)). This change in oxidation state indicates that zinc has lost electrons.

Oxidation is the process in which an atom, ion, or molecule loses electrons. In this reaction, zinc has lost two electrons, which is equivalent to an oxidation state change of +2.

Now, let's complete the half equation to show the oxidizing action of bromine. The half equation for the oxidation of iodide ions by bromine is:

2I-(aq) -> I2(aq) + 2e-

In this equation, two iodide ions (I-) are oxidized to form one molecule of iodine (I2) while releasing two electrons (2e-). The bromine (Br2) acts as an oxidizing agent as it causes the oxidation of iodide ions.