Question

Could someone help me out with this question? i'm a little stuck

Balance the following redox equation using the oxidation number change method. Describe each step that is involved (each step 1 points) Correct oxidation numbers assigned (1 point) Correct balanced equation (1 point) Al(s) + PbSO4 - - > Al2(SO4)3 + Pb(s)

Answer 1

@JFraser any idea?

Answer 2

the method I use isn't called the "oxidation number change method", but I'd guess they all do pretty much the same thing.

You need to look at each piece of each formula, and figure out what the charge of each atom or ion is. For example, an \(element\) by itself always has an oxidation state of zero

A \(compound\) has a total oxidation number of zero, but it's made up of charge pieces, so we look at the periodic table to figure out what ions are making what charges

Answer 3

So

Al= +3
PbSO4= +2

Answer 4

@Ebonygotthejuice Could you help me finish this?

Answer 5

i have no idea at all im sorry

Answer 6

when an element is \(not\) part of a compound, its oxidation is zero, so the reactant \(Al(s)\) has a charge of 0