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Question

# (a) (i) Calculate the volume of 320 of SO2 at STP. (Atomic mass : S = 32 and O = 16). (ii) State Gay-Lussac's law of combining volume (iii) Calculate the volume of oxygen required for the complete combustion of 8.8 g of propane (C3H8) (Atomic mass; C = 12, 0 = 16, H = 1, Molar volume −22.4dm3 (b) (i) An organic compound with vapour density = 94 contains C = 12.67% H = 2.13 % and Br = 85.11% Find the molecular formula. [Atomic mass ; C = 12, H = 1, Br = 80] (ii) Calculate the mass of (1) 1022 Atoms of sulphur. (2) 0.1 mole of carbon dioxide. [Atomic mass; S = 32, C = 12 and O = 16 and Avogadro's number =6×1023

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Solution

## (b) (i) Element Relative atomic mass %compound atomic ratio Simple ratio H 1 2.13 2.131=2.13 2 C 12 12.67 12.6712=1.055 1 Br 80 85.11 85.1180=1.063 1 Empirical formula = n × (Empirical formula mass of ) = Molecular mass [2 × V.D] n(12+2+80) = 94× 2 n = 2 molecular formula =2 × Empirical formula =

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