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September 20, 2014

September 20, 2014

Posted by **M** on Sunday, October 7, 2012 at 12:26pm.

Current annual energy consumption in the United States is 99.3 quads. Assume that all this energy is to be generated by burning CH4(g) in the form of natural gas. If the combustion of the CH4(g) were complete and 100% efficient, how many moles of CH4(g) would need to be combusted in order to provide the U.S. energy demand?

I am clueless as to how to solve this. My teacher did not go over this material so if someone could show me step by step how to solve this, that would be very much appreciated!!

- Chemistry -
**DrBob222**, Sunday, October 7, 2012 at 3:56pmYou want to check my work very carefully. The long way of doing this is to write and balance th equation, and use stoichiometry to calculate grams CH4 need then convert that to mols. I've tried a shorter route and if you use it you may learn how to shorten some calculations also.

First I went to google and let google convert 99.3 quads BTU to megajoules. That's about 1.05E12 MJ. Then I found a page on the internet that gave the combustion of CH4 to be 38 megajoules/cubic meter. Google converts 1 cubic meter to 1000 L and 1000 L/22.4 L/mol = about 44/6 mols so 38 MJ/m^3 = 38 MJ/44.6 mol.

38 MJ/44.6 mol x # mols = 1.05E12 MJ.

And solve for # mols.

If you haven't used google for conversions yet, try it. For example covert 22.4 L to cubic meters. Type in the google window "22.4 L to cubic meters" without the quotation marks and hit the enter button. You will get the answer that 22.4L = 0.0224 cubic meters.

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