At $300K$ and 1 atmospheric pressure, $10mL$ of a hydrocarbon required $55mL$ of $O_2$ for complete combustion and $40mL$ of $C{O}_2$ is formed. The formula of the hydrocarbon is:

Q. 20 ml of a hydrocarbon requires 100ml of oxygen under the same conditions for complete combustion 60 ml of $C{O}_2$ is formed. The formula of hydrocarbon is:

Q. At 300 K and 1 atm, 15 mL of a gaseous hydrocarbon requires 375 mL air containing 20% $O_2$ by volume for complete combustion. After combustion the gases occupy 330 mL. Assuming that the water formed is in liquid form and the volumes were measured at the same temperature and pressure, the formula of the hydrocarbon is:

Q. $20$ ml of a hydrocarbon requires $100$ ml of oxygen for complete combustion. In this reaction, $60$ ml of carbon dioxide is produced. The formula of hydrocarbon is:

Q. $V\text{mL}$ of a hydrocarbon $C_x{H}_y$ requires $6V\text{mL}$ of oxygen for complete combustion & forms $4V\text{mL}$ of $C{O}_2.$ The value of $y$ is .

Q. 100 ml of a hydrocarbon on combustion gave 300 ml of $C{O}_2$ and 400 ml of water vapor measured under similar conditions of temperature and pressure. Find out the molecular formula of hydrocarbon.