Posted by Sarah on Wednesday, November 12, 2008 at 8:04pm.
q = mass air x sp. h. air x delta T will give you the heat required in J. Since sp. h. of air is given in J/mol*K, you need to convert mass of air to mols air using the mass/mol of 28.9 g/mol. What's missing from the problem is the heat generated by the combustion of CH4 and you need that before you can get grams of CH4. Perhaps its in the problem or you can look it up somewhere. As for the O2 or air, you are heating air but you are burning O2. My take on the problem is that the combustion of CH4 does not depend upon the air in the room but the air for the combustion is coming from another source. So whether it's oxygen or air mixed with oxygen need not enter into the problem. I would think either volume or grams would do for the amount of CH4. I would go with grams if I had a choice but I don't have a reason for that choice.
I found on another website that the heat of the reaction of CH4 is 50.1 kj/kg. Can this number be used in my question as well? I dont know where else to find this information.
After I get this information what do I need to do? Which formula is needed?
Thank you for your help so far!
I found on another website that the heat of the reaction of CH4 is 50.1 kj/kg. Can this number be used in my question as well? I dont know where else to find this information.
After I get this information what do I need to do? Which formula is needed?
Thank you for your help so far!
heat needed is mass air x sp. h. air x delta T. You have the MOLAR specific heat of air so you need to change the volume to grams to mols. Calculate q.
CH4 + 2O2 ==> CO2 + 2H2O + 50.1 kJ/kg heat generated.
Knowing q (in J/g) and the reaction produces 50.1 kJ/kg, calculate grams CH4 needed. (By the way, since delta T is a difference, it makes no difference if you subtract C from C or K from K, the difference is 7 degrees.)
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