What is the volume in liters of SO2 gas needed to completely consume 1.40 kg of H2S if the density of SO2 is 2.279 kg per m3?

Answer 1

Though there is no common reaction known of how to 'consume' (whatever that may be: H2S and SO2 are both very toxic!) hydrogen sulfide, one might deduce the molar reaction ratio of H2S to SO2 from the 1 to 1 atomic sulfur content, this gives us equal amounts in moles H2S and SO2.

Since 1.40 kg H2S equals 1.40(kg) / 0.03418(kg/molH2S) = 40.96 mole H2S one can easily calculate that the same amount SO2 weights 40.96(molSO2) * 0.06407(kg/molSO2) = 2.62 kg SO2 which equals 2.62(kgSO2) / 2.279(kg/m3) = 1.15 m3 SO2 gas

Molar masses: 0.03418 kg/mol H2S and 0.06407 kg/mol SO2

Answer 2

First, calculate the volume of 1.40 kg of H2S by dividing its mass by its density (density of H2S is around 1.43 kg/m3) to get the volume in cubic meters. Then, using the stoichiometry of the reaction between SO2 and H2S, determine the molar ratio needed to completely consume H2S. Finally, use the molar volume at standard temperature and pressure (around 22.4 L/mol) to find the volume of SO2 gas in liters.