How many grams of H2 are needed to produce 10.41g of NH3

How many molecules (not moles) of NH3 are produced from 7.94×10−4 g of H2?

Balanced Equation: N2 + 3 H2 --> 2 NH3

10.41 grams NH3 X (1 mol/17.00 grams) = 0.612 moles NH3 X (3 mol H2 / 2 mol NH3) = 0.918 moles H2
0.918 mol H2 X 2.01 g/mol = 1.85 grams H2 required

7.94 X 10^-4 g H2 X (1 mol/2.01 grams) = 0.93.95 X 10^-4 mol H2 X (2 mol NH3 / 3 mol H2) = 2.63 X 10^-4 moles NH3
2.63 X 10^-4 moles X 6.02 X 10^-23 molecules/mol = 1.58 X 10^20 molecules NH3