Wednesday
June 19, 2013

# Homework Help: chemistry

Posted by Sarah on Wednesday, November 12, 2008 at 8:04pm.

You want to heat your house with natural gas CH4. The house has 275 sq. m of the floor area and the height of 2.5 m (between the floor and the ceiling). The air has a specific molar heat capacity of 29.1 j/mol*K. The molar mass of air is 28.9 and a density of 1.22 g/L at these temperatures. How much methane do you have to use in order to heat air from 15 to 22 oC in your house?

I changed the temperatures to Kelvin, so they are now 288K and 295K. I also found the volume by multiplying 275 by 2.5 = 687.5. And that means that the mass of air is 838.75. After that Im stuck.

Do I use PV=nRT? or q = s * m * change in t?

Also, am I looking for grams of methane? Or volume? Or mass?

And, the problem only says "air"... Does that mean O2?

Im sorry for all the questions! Thank you for the help though!

• chemistry - DrBob222, Wednesday, November 12, 2008 at 8:42pm

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.

• chemistry - Sarah, Wednesday, November 12, 2008 at 9:02pm

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!

• chemistry - Sarah, Wednesday, November 12, 2008 at 9:10pm

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!

• chemistry - DrBob222, Wednesday, November 12, 2008 at 10:26pm

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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