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A sample of a compound consists of C , H and N only.If 24 gm of carbon , 6.022 x 1024 atoms of hydrogen and 2 -gm atom of nitrogen is present and vapour density of the compound is 16.5 , then its molecular formula will be ?
vapor density is 16.5
=> molecular mass should be 16.5 * 2 = 33
Now it has 24 gm carbon => 2x moles of carbon
2-gm atom of N = 2x moles of nitrogen
.
going this way the empirical mass> molecular mass
that immpossible
you posted a wrong question
check again!!
given vapour density=16.5so molecular mass= 2.d=33 gmno. of moles of carbon=2no. of moles of hydrogen=10moles of nitrogen=2,ratio of moles=2:10:2=1:5:1but according to this the mass comes=31 gm.hence the no of hydrogen req. more=2so the formula becomes.... CH(7)N
the method i try to remove empirical formula
is it CH5N
vapour density = molecular mass/2
so ur ans is....16.5*2 = 33g/mol
CH5N
wrong question
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