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How to find the empirical formula?

How to find the empirical formula of lead sulphide?

  • Answer:

    Pb + xS → PbSx 2.46.......→ 3.22 g of product so mass of S = 3.22 -2.46 = 0.76 g %S = 0.76/ 3.22 × 100 = 23.60 %Pb = 2.46/ 3.22 × 100 = 76.40 (phew they add to 100% that was lucky!) Atomic ratios: Pb = 76.40/207.2 = 0.37; S = 23.60/32.07 = 0.74 Empirical formula is PbS2 I checked and PbS2 is known and prepared this way; so I've learned today! http://en.wikipedia.org/wiki/Lead%28IV%29_sulfide

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Pb + xS → PbSx 2.46.......→ 3.22 g of product so mass of S = 3.22 -2.46 = 0.76 g %S = 0.76/ 3.22 × 100 = 23.60 %Pb = 2.46/ 3.22 × 100 = 76.40 (phew they add to 100% that was lucky!) Atomic ratios: Pb = 76.40/207.2 = 0.37; S = 23.60/32.07 = 0.74 Empirical formula is PbS2 I checked and PbS2 is known and prepared this way; so I've learned today! http://en.wikipedia.org/wiki/Lead%28IV%29_sulfide

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