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jkp269
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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. Thankyou.
A natural gas mixture is burned in a furnace at a powergenerating 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
 one year ago
 one year ago
jkp269 Group Title
This question is driving me crazy. I don't necessarily want all of the steps, just a push in the right direction. Thankyou. A natural gas mixture is burned in a furnace at a powergenerating 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
 one year ago
 one year ago

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joemagee Group TitleBest ResponseYou've already chosen the best response.1
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.
 one year ago

jkp269 Group TitleBest ResponseYou've already chosen the best response.0
Ok, so bond enthalpies, not standard enthalpies of formation?
 one year ago

joemagee Group TitleBest ResponseYou've already chosen the best response.1
You can use standard enthalpies of formation as well. They should give you approximately the same answer.
 one year ago
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