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

Chemistry

1 answer:

goldenfox [79]4 years ago

8 0

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?

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