2C2H6 + 7O2 --> 4CO2 + 6H2O
dGrxn = (n*dGo products) - (n*dGo reactants)
use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 moles of ethane, CH3CH3(g), at 25 °C and standard conditions.
on the chart is said ethane(C2H6) is -84.0.
In the hint it said deltaGf is -30.2 kJ/mole, but then I can't find it on the chart nor do I know now to start the problem. I just know that it is delta G rxn = delta G (products)- delta G(reactant). There is no equation am I supposed to just take product as G(CH3CH3) and subtract 2G(C) and 3G(H2). Please help! Thank you.
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