Answer to Question #155527 in Inorganic Chemistry for David Perdomo

Question

Tarnishing of silver is caused by small amounts of hydrogen sulfide released into the atmosphere by decaying organic material and volcanic activity. According to the following equation:

 4Ag(s) + 2H₂S(g) + O₂(g) → 2Ag₂S(s) + 2H₂(l)

How many grams of Ag₂S can be produced from 1.70g H₂S if sufficient amount of the other reactants are present?

Answer 1

The molar masses are:

$M_{Ag_2S}=247.8g/mol$

$M_{H_2S}=34.1g/mol$

Therefore,

$m_{Ag_2S}=1.70g_{H_2S}\times\frac{1mol_{H_2S}}{34.1g_{H_2S}}\times\frac{2mol_{Ag_2S}}{2mol_{H_2S}}\times\frac{247.8g_{Ag_2S}}{1mol_{Ag_2S}}=12.4g$

Answer: 12.4 g