Question
Mon May 16, 2011 By:

Nine volumes of gaseous mixture consisting of a gaseous organic compound A and just sufficient amount of oxygen required for complete combustion yielded on burning 4 volumes of CO2 , 6 volumes of water vapour and 2 volumes of N2 all volumes measured at the same the same temprature and pressure. If the compund A contained carbon, hydrogen and nitrogen- 1)How many volumes of oxygen are required for complete combustion? 2)What is molecular formula of the compound A?

Expert Reply
Fri June 24, 2011
  The balanced chemical equation can be written as:-
    C2H4N2 + 3O2 ? 2CO2 + 2H2O + N2
     (9-v)        v            4         6        2
 
(i) The GAY LUSSAC'S LAW ,according to which the reactants are in whole number ratio which is equal to the mole ratio.
   (9-v)/v=1/3
  27-3v=v
   27=4v
   v=6.75mL
 
(ii) The molecular mass of compound A i.e. C2H4N2=(2×12)+(4×1)(2×14)=56g/mol.
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