Question

4.12 grams of Zinc are placed in a crucible with 3.00 grams (excess) of Sulfur. when reaction is complete the product mass is 6.10 grams. What mass of Sulfur should be used in the simplest formula calculation? Find the empirical formula of Zinc Sulfide.

My work...
6.10 g Product - 4.12 g Zn = 1.98 g S

4.12 g Zn • (1 mole Zn)/(65.38 g Zn) = 0.063 moles Zn

1.98 g S • (1 mole S)/(32.06 g S) = 0.062 moles S

1.98 g Sulfur should be used in simplest formula calculation.

Making the simplest empirical formula ZnS because the moles are basically the same so the mole ratio is one to one....

Please let me know if this is right and if not please show me where I went wrong...

Answer 1

the mole ratio is very nearly 1:1, so your answer seems good.