If two mole of H2S and 11.2 dm³ of SO2 at STP react according to the following equation SO2+2H2S---2H2O+3SWhat will be the number of moles of sulphur formed in the reaction?
Correct answer: A. 1.5
- A. 1.5
- B. 11.2
- C. 3
- D. 6
Explanation
1mol => 22.4dm3 at STPxmol => 11.2dm3 at STPx= 0.5molSO2+2H2S---2H2O+3S1mol. 2mol. 3mol0.5mol 2mol. xmolAs SO2 is the limiting factor hence further calculation will be with SO21mol => 3mol0.5mol => xmolx= 1.5mol
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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