Chemistry Question? Carbon Hydrogen Question

Please help with this question.
A 2.524 g sample of a compound contains carbon hydrogen and oxygen. Carbon hydrogen analysis reveals 3.703 g of carbon dioxide and 1.514 g of water are produced. If one mole contains 7.224 x 1024 atoms of hydrogen determine the molecular formula.
I can get all the way to finding the empirical formula but then the one mole contains 7.224 x 10 to the 24 atoms throws me off. Please help and explain, Thanks!

Let us check the empirical formula - what a pity you did not provide you answer for this because it would make things much easier for answerers.

mass C in 3.703g CO2 = 12/44*3.703 = 1.01
Mass H in 1.514g H2O = 2/18*1.514 = 0.168
Mass O in sample = 2.524 - ( 1.01+0.168) = 1.346

Divide each by respective atomic mass:
C = 1.01*12 = 0.084
H = 0.168/1 = 0.168
O = 1.346/16 = 0.084

Empirical formula = CH2O
Now to work out the molecula formula:
You know that 1 mol of the empirical formula will contain 6.022*10^23 formula units, and because each formula unit contains 2H atoms, there will be
2*6.022*10^23 = 1.2044 * 10^24 H atoms in 1 mol of the formula units

But 1 mol of the compound contains 7.224*10^24 H atoms
Therefore each molecule of the compound will contain : (7.224*10^24) / 1.204*10^24) = 6 H atoms

The empirical formula contains 2 H atoms in CH2O
The molecular formula will be (CH2O) * 6/2 = (CH2O)3 = C3H6O3

that is not too difficult but I don't know how to write at here.
so I'm so sorry