Question: Determine the reaction enthalpy for the hydrogenation of ethyne to ethane, C2H2(g) + 2 H2(g) --> C2H6(g), from the following data: deltaHc(C2H2, g) = -1300. kJ/mol, deltaHc(C2H6, g) = -1560. kJ/mol, deltaHc(H2, g) = -286 kJ/mol.
I was able to do this problem, but my answer does not match the solutions manual. Can someone help me with this to see where I went wrong please? Thank you!
Question 8.57 (Sixth Edition)
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Re: Question 8.57 (Sixth Edition)
I'm having trouble with this too... I did the sum of the standard enthalpy of combustion for products - reactants but I got +312 kJ instead of -312 kJ. I know it should be negative because it's a combustion reaction, thus exothermic, but that math doesn't match up.
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Re: Question 8.57 (Sixth Edition)
I am also confused about this problem. My answer doesn't match the solutions manual either.
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- Posts: 37
- Joined: Mon Apr 23, 2018 3:00 am
Re: Question 8.57 (Sixth Edition)
viewtopic.php?t=17644
I found this thread that explains how to do the problem well. Essentially, you have to find the combustion reaction for each element of the given reaction and then use method 1 for solving for enthalpy to find the reaction enthalpy for the hydrogenation of ethyne to ethane.
I found this thread that explains how to do the problem well. Essentially, you have to find the combustion reaction for each element of the given reaction and then use method 1 for solving for enthalpy to find the reaction enthalpy for the hydrogenation of ethyne to ethane.
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