A natural gas may be assumed to be a mixture fo methane and ethane only. On complete combustion of `10L` of gas at `STP` the heat evolved was `474.6 kJ`. Assuming `Delta_(comb) H^(Theta) CH_(4)(g) =- 894 kJ mol^(-1)` and composition of the mixture by volume.

A natural gas may be assumed to be a mixture of CH_4 and C_2H_6 only. On complete combustion of 10 L of the gas at STP, the heat evolved was 474.6 kJ. Assuming DeltaHc(CH_4) = – 894 kJ//mol and " "DeltaHC(C_2H_6) = - 1560 kJ//"mole" . Calculate the % by volume of each gas in the mixture

3L Mixture of propane and butane on complete combustion at 298K and 1atm gave 10L CO_2. Calculate the composition of gas

A gas mixture of 3.67 lit of ethylene and methane on complete combustion at 25^@C and at 1 atm pressure produce 6.11 lit of carbon dioxide. Find out the amount of heat evolved in kJ, during this combustion. ( DeltaH_C(CH_4)=-890 "kJ mol"^(-1)) and (DeltaH_C(C_2H_4)=-1423 "kJ mol"^(-1)) .

The heat librerated on complete combustion of 1 mole of CH_(4) gas to CO_(2)(g) and H_(2)O(l) is 890 kJ. Calculate the heat evolved by 2.4 L of CH_(4) on complete combustion.