205 gram hydrogen sulfide reacts with 75.0 g oxygen to produce sulfur and water. Find: a) Gram of sulfur formed b) gram of excess reactant used up c) gram of excess reactant that remained unreacted

Md Ariful Islam

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H2S + O2 --->>H2O + S

Molar mass of H2S = 34.1

= 205/34.1 = 6.0112 moles

Molar mass of oxygen = 31.998

75/31.998 = 2.344 moles

Mole ratio in both cases = 1:1

= 2.344+6.0112 = 8.3552 moles of Sulfur

Molar mass of sulfur = 32.065

= 32.065 × 8.3552 = 267.91g of sulfur

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