22.4 litres of a gas weighs 70 g at S.T.P. Calculate the weight of the gas if it occupies a volume of 20 litres at $27^{\circ} C$ and 700 mm Hg of pressure.

^{'} x^{'}

moles of

N_{2}

gas at S.T.P. conditions occupy a volume of 10 litres, then the volume of

^{'} 2 x^{'}

moles of

C H_{4}

273^{o} C

and 1.5 atm is:

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Calculate the volume occupied by 40 g. of a CH4 at S.T.P if its V.D. is 8.

The correct option is C 56 litresMolar mass =2×vapour density=2×8=16gmNo of moles =4016=2.5So volume =2.5×22.4=56 litres

Calculate the volume occupied by 40 g. of a $C H_{4}$ at S.T.P if its V.D. is 8.

The correct option is C 56 litres
Molar mass $= 2 \times v a p o u r d e n s i t y = 2 \times 8 = 16 g m$
No of moles $= \frac{40}{16} = 2.5$
So volume $= 2.5 \times 22.4 = 56 l i t r e s$