Hello aspirant,
First we have to calculate the molar mass of organic compound having an empirical formula, CHBr
using ideal gas equation:
PV=nRT
where,
P = pressure of gas = 752 mm Hg = 0.989 atm
conversion used : (1 atm = 760 mmHg)
V = volume of gas = 24.2cm^3=24.2ml=0.0242L24.2cm3=24.2ml=0.0242L
conversion used :
(1cm^3=1ml)
(1L=1000ml)
(1cm3=1ml)
T = temperature of gas = 14^oC=273+14=287K14oC=273+14=287K
R = gas constant = 0.0821 L.atm/mol.K
w = mass of an organic compound = 0.188 g
M = molar mass of an organic compound = ?
Now put all the given values in the ideal gas equation, we get:
(0.989atm) * (0.0242L)=[{0.188g}/{M}] * (0.0821L.atm/mol.K)* (287K)
M=185.08g/mole
The Empirical formula = C H Br
The empirical formula weight = 12 + 1 + 80 = 93 gram/eq
Now we have to calculate the valency factor.
Formula used :
n= {Molecular formula}/{Empirical formula weight}}= {185.08}/{93}=1.99≈2
Molecular formula = (C H Br)n=(C H Br)2=C2H2Br2
Therefore, the molecular of the compound is, C2H2Br2.
Hope, this helps you.
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