Empirical Formula of Epsom Salt

My question says.

Epsom salt contain 9.86% magnesium, 13.02% sulfur, 71.43% oxygen and 5.68% hydrogen.

I know to take each of these from percent to grams and then divide by their atomic mass but I do not think my ratios are right so if someone could go through the steps it would be very helpful.

I know that epsom salt is MgSO4 so don't just post the answer, please explain the steps.

First of all, you're right epsom salt MgSO4 but the problem says it contains hydrogen so they're probably talking about MgSO4*7H2O which is the hydrous form. Anyhow, we'll figure it out.

We convert to moles since the empirical formula, or any formula for that matter, is the ratio of MOLES! (btw a periodic table is essential to solve these problems)
9.86 g Mg / 24.31 = 0.406 mol Mg (remember! keep your significant digits)
13.02 g S / 32.07 = 0.4060 mol S
71.43 g O / 16.00 = 4.464 mol O
5.68 g H / 1.008 = 5.63 mol H

Now lay them out in a ratio form... remember the order (Mg : S : O : H)
0.406 : 0.4060 : 4.464 : 5.63
Next divide everything by the smallest # (.406 in this case) It gets the smallest # to 1 and everything else above 1 to make the next steps easier.
1.00 : 1.00 : 11.0 : 13.9
if you can see that everything is really close to a whole number, go ahead and round
(but for example if it wasn't say like 1 : 1.5 , you would multiply everything by 2 to make the 1.5 a whole number and the ratio to 2 : 3)

finally we have
1 : 1 : 11 : 14
since this is a hydrous compound (water attached to it) and there's no hydrogen in the actual formula, we can assume that all the hydrogen belongs to the attached water and since H2O has a 2:1, H:O ratio, we have to assume that 7 of the oxygens are together with the 14 hydrogens

1 : 1 : 4 * 7H2O
the rest is trivial
MgSO4 * 7H2O
there ya go!