The thermal decomposition of 1.6608 g of MgSO4 * H2O produces 1.4446 g of a

Question

product in a well-behaved reaction. There are two possibilities:

1) MgSO4 * H2O(s) -> MgSO4(s) + H2O(g)

2) MgSO4 * H2O(s) -> MgO(s) + SO3(g) + H2O(g)

Complete the following table, and then identify the correct solid product by
comparing the calculated masses of MgSO4 and MgO with the observed mass of
the product.

Formula
Substance Weight Moles Mass (g)
-----------------------------------------------------

MgSO4 * H2O __________ __________ __________

MgSO4 __________ __________ __________

MgO __________ __________ __________

Because the observed mass of the product is 1.4446 g, the product is
__________.

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** HERE'S HOW I COMPLETED THE TABLE **
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Formula
Substance Weight Moles Mass (g)
-----------------------------------------------------

MgSO4 * H2O _138.4____ _0.0120___ _1.6608___

MgSO4 _120.4____ _0.0120___ _1.4446___

MgO __40.31___ _0.0358___ _1.4446___

I'm not sure if I did this correctly if I didn't can someone plz exaplin which part and how to do it

Thank You

Answer 1

You have it. So MgSO4 was the product, because you have to end up with the same number of moles of Mg as you started with.