Chemistry

Enthalpy
I'm given that the heat of reaction for the combustion of ethane is -1560kJ/mol. I need to figure out how much heat is produced from 18g of ethane.
2 C2H6 + 7 O2 --> 4 CO2 + 6 H2O

Okay so I'm rough on Thermo right now, so I gave it my best shot. Could we write each molar amount from the equation as equal to the heat of reaction:
2mol ethane = -1560kJ/mol
7mol oxygen gas = -1560kJ/mol
4mol carbon dioxide = -1560kJ/mol
6mol water = -1560kJ/mol

Then could I convert the given 18g of ethane into moles and convert to the heat produced, using -1560kJ/mol as the heat converting value:
(18g ethane)/(30.07g/mol ethane) = .599mol ethane
(.599mol ethane)/(2mol ethane)*(-1560kJ/mol ethane) = -467.22kJ

Okay so my previous problem was going to be the fact that my final answer was -279.7kJ instead of -467.22kJ (my computer calculator doesn't show history so I don't know what dumb thing I did!)

However, here are the answers available:
A) -220.5kJ
B) -466.75kJ
C) 300.21kJ
D) 424.67kJ

So the right answer is B? Ethane, or 18g of ethane, releases about 467.22kJ or 466.75kJ? Or do these two values vary too much as to refute my calculations?

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