Let the formula of unknown organic compound be CxHyOz. Let the combustion of the organic compound be
CxHyOz + O2 = CO2 + H2O
Applying POAC(principle of atomic conservation) on each atom of the above reaction which says that number of atoms of an element in a chemical reaction remains conserved.
Given,
Mass of unknown organic compound = 4.989 g
Mass of H2O produced=2.284 g
Mass of CO2 produced=7.438 g
Molar mass of unknown organic compound = 118.1 g/mol
Moles of unknown organic compound , n1 =
mass of unknown compound /molar mass of unknown organic compound
Moles of unknown organic compound , n1 = 4.989 /118.1
n1=0.0422 mol
Moles of H2O , n2= mass of H2O/molar mass of H2O
n2=2.284/18
n2= 0.1269 mol
Moles of CO2 ,n3= mass of CO2/molar mass of CO2
n3= 7.438/44
n3= 0.1690 mol
Applying POAC on carbon atoms,
1 mole of CxHyOz contains x mole atoms of C
0.0422 mole of CxHyOz contains 0.0422x mole atoms of C
0.0422x atoms of C will be in reactant side.
1 mole of CO2 contains 1 mole atoms of C.
0.1690 mole of CO2 contains 0.1690 mole atoms of C.
Number of atoms of C in reactant is equal to number of C atoms in product side.
0.0422x=0.1690
x=4.0047= 4
Applying POAC on hydrogen atoms ,
1 mole of CxHyOz contains y atoms of H
0.0422 mole of CxHyOz contains 0.0422y mole atoms of H
0.0422y atoms of H will be in reactant side.
1 mole of H2O contains 2 mole atoms of H
0.1269 mole of H2O contains 0.2538 mole atoms of H
Number of atoms of H in reactant side will be equal to number of atoms of H in product side.
0.0422y=0.2538
y=6.0142=6
We will not apply POAC on oxygen atoms because oxygen atoms are present in excess.
Given, molar mass of CxHyOz =118.1 g/mol
Also, molar mass of CxHyOz is equal to
x*molar mass of C + y*molar mass of H + z*molar mass of O
x*12+y*1+z*16
4×12+6×1+z*16=118.1
54+z*16=118.1
z*16=64.1
z=4.00625=4
Hence, x=4,y=6,z=4
Molecular formula= C4H6O4
highest common factor of x,y,z is 2. Hence,
Empirical formula= C2H3O2
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