Chemistry percent yield

The decomposition of Pb(NO3)2 produces PbO, NO2, and O2 with a 89% yield. If a 4.30 g sample of Pb(NO3)2 is heated, what mass of PbO is actually produced?

Here is the balanced equation:
2Pb(NO3)2 = 2PbO + 4NO2 + O2

I've been working on this for hours and I can't figure it out :(( please if anyone can give me ANY kind of help it would be greatly appreciated.

2Pb(NO3)2 = 2PbO + 4NO2 + O2

Molecular Weight Pb(NO3)2 = 331.27

Molecular Weight PbO = 223.21

Use the following relationship:

4.3/(2x331.27) = x/(2x223.21) x = 2.90

The theoretical yield is 2.90. The yield is:

89/100 = x/2.9 x = 2.58 grams

from the balanced equation find the number of moles of reactant that produces no of moles of product

then from 4.3g of reactant, covert that into moles of reactant used

use that to find the moles of product created and convert that to grams...this is the theoretical yield

using formulae %yield = (tho. yield-actual yield) / theo. yield

we can get the actual yield which is what you need