I have a question from the Chemical Principles book. I don\'t necessarily want a

Question

I have a question from the Chemical Principles book. I don't necessarily want all of the steps, just a push in the right direction. Thank-you. <?xml:namespace prefix = o ns = "urn:schemas-microsoft-com:office:office" /?>

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 the information that I have. I found the standard enthalpies of formation in the Appendix, but again, I can't figure out how to use them to find the heat.

Explanation / Answer

we should consider combustion of each reactions i.e combustion of CH4 , C2H6, C3H8 , C4H10 and find out stociometrically amount of CO2 produced with moles given b) Molar enthalphy of each reaction can be found out text books or web. based on moles given we can calculate enthalphy i.e heat produced for each reaction. We can sum these to find total heat released.

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