To identify the hydrocarbon, we need to calculate the number of carbon and hydrogen atoms in the given molecule and then compare it with the possible hydrocarbons.



10 ml of hydrocarbon on combustion gives 40 ml of SeO2 gas and 50 ml of H2O vapours.

From the equation of combustion of hydrocarbon, we know that the number of moles of CO2 formed is equal to the number of moles of hydrocarbon combusted.

We can use this information to calculate the number of moles of hydrocarbon combusted and then use it to find the empirical formula of the hydrocarbon.



Let the number of moles of hydrocarbon be x.

The volume of SeO2 gas formed is 40 ml. We know that 1 mole of gas occupies 22.4 L at STP.

Therefore, the number of moles of SeO2 gas formed = (40/1000) / 22.4 = 0.000893 moles

From the balanced equation of combustion of hydrocarbon, we know that 1 mole of hydrocarbon reacts with 4 moles of SeO2 gas.

Therefore, the number of moles of hydrocarbon combusted = 0.000893 / 4 = 0.000223 moles



The number of moles of hydrogen atoms in the hydrocarbon = 2 x the number of moles of water vapour formed = 2 x (50/1000) / 22.4 = 0.001116 moles

The number of moles of carbon atoms in the hydrocarbon = 1/2 x the number of moles of SeO2 gas formed = 1/2 x (40/1000) / 22.4 = 0.000446 moles

Therefore, the empirical formula of the hydrocarbon is C2H5.



The hydrocarbon is C2H5, which is ethane.

Arey, usne options last me diya hai, dhyan se dekh... correct answer is C4 H10