The value of delta H for the reaction
C3H8(g) + 5O2(g) ---> 3CO2(g) + 4H2O(l)
delta H = -2220kJ\mol rxn
How much heat is given off when 33.0g of propane gas (C3H8) is burned at constant pressure?
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I first started off by calculating the number of moles present from propane:
33.0\44.094= ~0.7484 mol propane
I then was going to use the equation:
delta H = delta U + n*R*delta T
But there is no specified T, and delta U (the internal energy) could also be heat given off by a system correct?
So do I just take the T out of the equation and just plugin delta H, n(moles), and the value for R? Or am I using the wrong equation altogether for this type of calculation? Any help in the right direction would be greatly appreciated.
Thanks.