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Question

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 C and 0.1 bar pressure. What is the molar mass of phosphorus?

Solution
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Given,

p = 0.1 bar

V = 34.05 mL = 34.05 × 103 L = 34.05 × 103dm3

R = 0.083 bar dm3K1mol1

T = 546°C = (546 + 273) K = 819 K

From the gas equation PV = w. RT / M, we get

M = w. RT/ Pv ……….

(1)The molar mass of phosphorus, M=wRTPV=0.0625×0.08314×8191×34.05×103=124.46g/mol.

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