(a) (i) Calculate the volume of 320 of SO2 at STP. (Atomic mass : S =

1.	(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
Answer» (a) (i) Calculate the volume of 320 of $S O_{2}$ 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 $(C_{3} H_{8})$ (Atomic mass; C = 12, 0 = 16, H = 1, Molar volume $- 22.4 d m^{3}$ (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) $10^{22}$ Atoms of sulphur. (2) 0.1 mole of carbon dioxide. [Atomic mass; S = 32, C = 12 and O = 16 and Avogadro's number $= 6 \times 10^{23}$

(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

Answer»

(a)

(i) Calculate the volume of 320 of $S O_{2}$ 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 $(C_{3} H_{8})$ (Atomic mass; C = 12, 0 = 16, H = 1, Molar volume $- 22.4 d m^{3}$

(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) $10^{22}$ Atoms of sulphur.
(2) 0.1 mole of carbon dioxide.
[Atomic mass; S = 32, C = 12 and O = 16 and Avogadro's number $= 6 \times 10^{23}$

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