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NCERT Class XI Chemistry States of Matter Solutions

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Question : 10 of 23
Marks: +1, -0
34.05 mL of phosphorus vapours weigh 0.0625 g at 546°C and 0.1 bar pressure. What is the molar mass of phosphorus?
Solution:  
Molar mass of phosphorus, M
m = Mass of phosphorus
M = mRTPV\frac{mRT}{PV} = 0.0625×0.083×819(0.1)×(34.051000)\frac{0.0625 \times 0.083 \times 819}{(0.1) \times \left( \frac{34.05}{1000} \right)} = 1247.74 g/mol
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