Question

Hi, the question is: in each reaction, identify what have been oxidised and reduced.

The equation is: 2Al + 3H2SO4 ---> Al2(SO4)3 + 3H2
I am confused about the Al2(SO4)3 I know what oxides and reductions us I just don't understant how Al2(SO4)3 balances out to O with the oxidation numbers. Please help!!!
Sulfuric acid exists in solution as H⁺ and HSO₄⁻ ions, but both react with Al metal to produce Al⁺³ ions and SO₄⁻² ions. The most accurate representation of what's going on is:
2Al(s) + 3H⁺ + 3HSO₄⁻ --> 3H₂(g) + 2Al⁺³ + 6SO₄⁻²
or as ...
2Al(s) + 3H₂SO₄(aq) --> 3H₂(g) + Al₂(SO₄)₃(aq)
Make that 6SO₄⁻² a 3SO₄⁻²
Thank you very much :)

Related Questions

I need help splitting this reaction into 1/2 reactions 3I2(s) + 2MnO2(s)+8 OH-(aq)<-> 6I-(aq)... One more problem with 1/2 reactions Pb(s) + PbO2(s) + 2H2SO4(aq)->2PbSO4(aq)+2H2O(l). How do y... 2Li^++2I^-==>2Li+I2 would 2I^- be oxidised and 2Li be reduced reaction? The equation for the reaction that occurs when lead(II) oxide is heated with coke in a blast furnace...