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OpenStudy (anonymous):
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.
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OpenStudy (anonymous):
find the combustion equation to ethane. then use the appendix in your book to calculate the change in G for the reaction (products-reactants). K equals exp( -(G) / RT). R and T relate to the standard conditions. K = exp^336.15. Does this sound right?
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