Question

Question #0853f

Answer 1

You can use it like this:

Explanation:

Equation:

`2Al_((s))+6HCl_((aq))rarr2AlCl_(3(aq))+3H_(2(g))`

Aluminium loses it's outer electrons:

`2Al_((s))rarr2Al_((aq))^(3+)+6e`

These are taken in by the hydrogen ions:

`6H_((aq))^++6erarr3H_(2(g))`

In this reaction the chloride ions are spectators - they take no part in the reaction.

Answer 2

If you want to be able to balance the equation using oxidation states, here's how...

Explanation:

First you need to work out the oxidation states of each element, notice the ones that have changed, work out how many electrons they have lost/gained. From there find the key number to balance the equation and from then on this trial and error.