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This question is driving me crazy. I don't necessarily want all of the steps, just a push in the right direction. Thank-you. A natural gas mixture is burned in a furnace at a power-generating station at a rate of 13.0 mol per minute. (a) If the fuel consists of 9.3 mol CH4, 3.1 mol C2H6, 0.40 mol C3H8, and 0,20 mol C4H10, what mass of CO2(g) is produced per minute? (b) How much heat is released per minute? So what immediately struck me is that part (a) could be determined by normal stoichiometric methods, but the rate part is confusing me. Also I am not sure how to get the heat from

Chemistry
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Since the information is given as a rate (gas mixture burnt at 13.0 mol per minute) when you calculate the mass of CO2 the answer will also be a rate. For the heat you will either need to use bond enthalpies (from tables) and calculate that.
Ok, so bond enthalpies, not standard enthalpies of formation?
You can use standard enthalpies of formation as well. They should give you approximately the same answer.

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