Let the volumes of CO,CH4, and N2 in the mixture be x ml, y ml, and (10-x-y) ml respectively. We ignore the volume of water formed in the combustion as it is a liquid and its volume is small. Nitrogen combusts only at very very high temperatures. So it remains unreactive.
2CO+O2⟹2CO2 CH4+2O2⟹CO2+2H2O
x ml x/2 ml x ml y ml 2 y ml y ml (liquid)
The volume of oxygen used: 2y+x2ml
Total volume of all gases before combustion =10+2y+x2ml
After combustion the total volume is: 10 ml
as CO2:x+y N2:10−x−y
Reduction in volume: 10+2y+x2−10=2y+x2=6.5ml
⟹4y+x=13ml --- (1)
When the mixture of CO2+N2 passes over KOH, all of CO2 is absorbed. Only N2 remains. Then the reduction of 7 ml corresponds to that of CO2.
⟹x+y=7ml --- (2)
Solving the two equations, x = 5 ml and y = 2 ml
Volumes of CO=5ml, CH4=2ml , N2=3ml.