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0.188 g of an organic compound having an empirical formula CH2Br displaced 24.2 cc of air at 14 degree Celsius and 752 mm pressure . Calculate the molecular formula of the compound ( Aqueous tension at 14 degree Celsius is 12 mm


vaibhavijoshi44 18th Nov, 2020
Answer (1)
Shruti Smaranika 18th Nov, 2020

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)

(1L=1000ml)

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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