two mole of H2S and 11.2 dm³ of SO2 at STP react according to the following equation SO2+2H2S---2H2O+3S What 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 STP xmol => 11.2dm3 at STP x= 0.5mol SO2+2H2S---2H2O+3S 1mol. 2mol. 3mol 0.5mol 2mol. xmol As SO2 is the limiting factor hence further calculation will be with SO2 1mol => 3mol 0.5mol => xmol x= 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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