Question

How many grams of H2S is needed to produce 18.00g of PbS if the H2S is reacted with an

Answer 1

Answer:

2.56 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

Explanation:

The balanced reaction is:

Pb(CH₃COO)₂ + H₂S → 2 CH₃COOH + PbS

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) they react and produce:

• Pb(CH₃COO)₂: 1 mole
• H₂S: 1 mole
• CH₃COOH: 2 moles
• PbS: 1 mole

In this case,  to know how many grams of H₂S are needed to produce 18.00 g of PbS, it is first necessary to know the molar mass of the compounds H₂S and PbS and then to know how much it reacts by stoichiometry. Being:

• H: 1 g/mole
• S: 32 g/mole
• Pb: 207 g/mole

The molar mass of the compounds are:

• H₂S: 2* 1 g/mole + 32 g/mole= 34 g/mole
• PbS: 207 g/mole + 32 g/mole= 239 g/mole

So, by stoichiometry they react and are produced:

• H₂S: 1 mole* 34 g/mole= 34 g
• PbS: 1 mole* 239 g/mole=   239 g

Then the following rule of three can be applied: if 239 grams of PbS are produced by stoichiometry from 34 grams of H₂S, 18 grams of PbS from how much mass of H₂S is produced?

$mass of H_{2} S=\frac{18 grams of PbS*34 grams of H_{2}S }{239 grams of PbS}$

mass of H₂S= 2.56 grams

2.56 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