what volume in liters of methane must be burned?

Question

Assume that 3.65 x 106 kJ are needed to heat a swimming pool. If this energy is derived from the combustion of methane (CH4) at standard conditions (25 oC and 1 atm) what volume in liters of methane must be burned?




The heat of combustion of methane is 889.967 kJ/mol. The density of methane is 0.0680 kg/

Answer 1

It's too bad you didn't include the entire density unit. Somehow I doubt that it's kg per 100 liters, which, based on the ref, would be correct. (6.7E-4 g/cm^3 or 0.67 g/liter or 0.067 kg/100 liters). I'd use that.
Divide the total energy required by the heat of combustion. The result M is the number of moles of methane required.
Calculate the MW of methane.
Multiply M * MW. This is MM, the mass of methane required in g.
Divide MM by density in g/liter. That's the answer in liters of methane.
I hope you can do this easy math yourself, and some point-hungry weed doesn't come and do it for you..

Answer 2

we can anticipate room temperature and tension. 4g of methane is a million/4 of a mole, ie 6dm3 (at room temperature and tension). this could require 12dm3 of oxygen gasoline for comprehensive combustion. So thjere isn't sufficient oxygen. If 5dm3 of CO2 is produced, then 5dm3 of methane replaced into used up, leaving 1dm3 over. So the yield is 5/6. however the tension and temperature might desire to be reported, and, possibly, that discern of 24 dm3 for the molar quantity replaced.