How many grams of H2S is needed to produce 18.00g of PbS if the H2S is reacted with an excess (unlimited) supply of Pb(CH3COO)2?

2.56g of H₂S

Explanation:

The reaction of H₂S with Pb(CH₃COO)₂ is:

H₂S + Pb(CH₃COO)₂ → 2 CH₃COOH + PbS

Where 1 mole of H₂S produce 1 mole of PbS

18.00g of PbS (Molar mass: 239.3g/mol):

18.00g of PbS ₓ (1mol / 239.3g) = 0.0752 moles of PbS

As 1 mole of PbS is produced from 1 mole of H₂S, moles needed of H₂S are 0.0752

As molar mass of H₂S is 34.1g/mol, mass in 0.0752moles is:

0.0752 mol H₂S ₓ (34.1g / mol) = 2.56g of H₂S

50.23 i believe is correct but don't quote me on that.