Stoichiometry problem?

Question

What is the limiting reactant when 19.9 g of CuO react with 2.02 g of H2 according to the following: CuO+H2 ---->Cu+H2O

Answer 1

Molar mass CuO = 79.5454 g/mol
Moles CuO = 19.9 / 79.5454 = 0.250

Molar mass H2 = 2.01588 g/mol
Moles H2 = 2.02 / 2.01588 = 1.00
the ratio between CuO and H2 is 1 : 1
CuO is the limiting reactant
H2 is in excess : moles H2 in excess = 1.00 - 0.250 =0.750

Answer 2

CuO + H2 = Cu + H2O

The molar ratios are all 1:1 :: 1:1
moles CuO
1 x Cu = 1 x 63.5 = 63.5
1 x O = 1 x 16 = 16
63.5 + 16 = 79.5 (Mr of CuO)
moles(CuO) = 19.9 / 79.5 = 0.25 mol (CuO)
moles (H2) = 2.02 / 2.014 = 1.003 mol(H2)

On a one-to-one basis of the molar ratios 0.25 mol(CuO) would only need 0.25 mol(H2) to fully react. As there are 1.003 mol(H2) hydrogen is in excess.
Hence the limiting reagent is the CuO Copper (II) Oxide.