Calculate the mass of 0.1 mole of carbon dioxide.

[Atomic mass: S = 32, C = 12 and O=16 and Avogadro's Number = 6 x 10²³]

Q.

Calculate the mass of
(i) 10²² atoms of sulphur,
(ii) 0.1 mole of carbon dioxide.

[Atomic mass: S = 32, C = 12 and O = 16 and Avogadro's Number = 6 × 10²³]

Q.

Calculate the mass of 10²² atoms of sulphur.

[Atomic mass: S = 32, C = 12 and O=16 and Avogadro's Number = 6 x 10²³]

Q.

(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 $\left(C_3{H}_8\right)$ (Atomic mass; C = 12, 0 = 16, H = 1, Molar volume $-22.4d{m}^3$

(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 $=6\times {10}^{23}$

Q. Calculate the number of moles of ethylene required to produce $44$g of carbon dioxide gas on its complete combustion.

Q.

Calculate the number of molecules in 12.8 g of sulphur dioxide gas. Take Avogadro's number as 6 × 10²³.
[S = 32, O = 16]