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Question

34.05 mL of phosphorus vapour weighs 0.0625 g at 546oC and 1.0 bar pressure. What is the molar mass of phosphorus?

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Solution

p=0.1bar\\
V=34.05mL=34.05×103L=34.05×103dm3R=0.083bardm3k1mol1
T=546°C=(546+273)K=819K

We can calculate the number of moles (n) by using the ideal gas equation : pV=nRT.
Replacing n by mM, where, m=mass=0.0625g
M=Molecularmass, which we need to find.

pV=mRTM

So,M=mRTPV=(0.0625X0.083X819)(0.1X34.05×103)

=1247.5gmol1


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