"Number of moles of organic compound" = 0.2612/106
=> n=2.4642xx10^-3mol
"Number of moles of "CO_2 = 0.8661/44
=> n= 0.0197mol
"Number of moles of " H_2O = 0.2250/18
=> n= 0.0125mol
The equation for the reaction is:
C_aH_b + a*b*O_2 -> a*CO_2 + b/2*H_2O
Mole ratio of CO_2:"organic compund"= 0.0197/(2.4642xx10^-3
= 8:1
This means 8mol of CO_2 is produced for burning 1mol of the organic compound. The value of a is therefore 8.
Mole ratio of H_2O: "organic compound" = 0.0125/(2.4642xx10^-3
~~5:1
This shows 5mol of H_2O is produced. So, b/2 = 5, therefore b is equal to 10.
Hence, the organic compound has molecular formula C8H10. It's empirical formula would hence be C_4H_5. The name of this compound is Xylene, or dimethyl benzene.
**n.b. this is not an orthodox method. If this question is asked in an exam, you may not be awarded any marks for using this method.
