Chem help

"1. write a balanced equation [showing all states, i.e., (s), (I), and (G)], under the conditions of the experiment, that represents the complete dehydration of the compound Na_2S ° 9H_2O

2. when a 1.5937 g sample of an uknown hydrate was dehydrated upon heating, 0.8788 g of the anhydrous salt remained
(a) what percent of the original compound was water?
(b) how many moles of water were driven off during heating?
(c)the formula weight of the anhydrous salt is 155.0 g/mol. determine the number of moles of the anhydrous salt"

1) Na2S*9H2O(l) + heat -> Na2S (s) + 9H2O (g)

2) (a) 0.8788/1.5937 *100 = 5514%
(b) 1.5937 - 0.8788 = (0.7149 grams)/(18.02 grams per mol) = 0.0397 moles
(c) (0.8788 grams)/(155.0 grams per mol) = 0.00567 moles

I think that is right. It has been a couple of years since I have had to care about sig figs.

perfect thank you 10/10

2a is 55.14%, missed the decimal. You're welcome.