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