An 18.5 g sample of tin (M = 118.7) combines with 10.0g of sulfur (M = 32.07) to form a compound. What is the empirical formula of this compound? 

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Molar mars in `g/(mol)`

`Sn= 118.7`

`S=32.07`

Amount of Sn  moles used `= 18.5/118.7 =0.156`

Amount of S moles used `= 10/32.07 =0.312`

Mole ratio

`Sn: S =0.156 : 0.312 = 0.156/0.156 : 0.312/0.156 = 1:2`

So the empirical formula  is `SnS_2`

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