Chemistry Help: total ionic and net ionic equation?

Question

Write the toal ionic and net ionic equations for this redox reaction: H2(g) + Al2O3(s) > Al(s) + H2O(l)

Answer 1

Actually, I thought the reaction went the other way.
The net equations are for the oxidized and reduced species. In each, electrons are balanced, and if there isn't enough water for the oxygen in cations with the reduced anion, H+ is included. So....
hydrogen is oxidized and Al is reuced.
For H,
H2(g) - 2e = 2H+
For Al
Al+3 + 3e = Al (s)
Mult H equation by 3 and Al equation by 2 and add.
3H2 + 2 Al+3 = 6H+ + 2Al
This is the total ionic eqtn. The oxygen goes along for the ride between the oxide of aluminun and the oxide of water (6H+ provides the H+ for 3H2O

Answer 2

we inspect the fees of each and every atom on the two facets Halogens consistently have a cost of -a million. Hydrogen merely approximately consistently have a cost of +a million different than while performing as a hydride (wherein case it has a cost of -a million). All chemical components have an entire cost of 0. Left HCl --> H has cost +a million, Cl has cost -a million Fe --> Fe has cost 0 precise FeCl2 --> Fe has cost +2, Cl has cost -a million H2 --> H has cost 0 Then we chop up all of those compounds to ions. 2H+ + 2Cl- + Fe --> Fe2+ + 2Cl- + H2 (notice that i did not chop up H2 - it is by technique of the fact H2 isn't an ionic compound.) it is the full ionic equation (a.ok.a. T.I.E.) Now to get the internet ionic equation (a.ok.a. N.I.E.), we take out the spectator ions (ions that don't replace in cost and don't do something - for this reason 'spectators'). for this reason, the spectator ions are the chloride ions. Taking those out, we get: 2H+ + Fe --> Fe2+ + H2 this is the N.I.E.