8.37

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Kayla Ikemiya 1E
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

8.37

Postby Kayla Ikemiya 1E » Tue Jan 16, 2018 10:24 am

How do you know how to find the enthalpy? I don't understand how they derived the answer in the solutions manual.

Kelly Kiremidjian 1C
Posts: 62
Joined: Fri Sep 29, 2017 7:04 am

Re: 8.37

Postby Kelly Kiremidjian 1C » Tue Jan 16, 2018 11:30 am

For part a, you know that the vaporization of 0.579 moles of Ch4 requires 4.76 kJ of heat, so all you have to do is divide the amount of heat by the moles to find the enthalpy (kJ/mol).
4.76 kJ/0.579 mol=8.22 kJ/mol

For part b it is very similar but instead of being given moles, you are given grams. In this problem, you must first convert grams to moles using the molar mass. The molar mass of C2H5OH is 46.07 g/mol. To get moles, divide 22.45 grams by 46.07 g/mol to get 0.4873 moles. Now you can do the same thing you did in part a. Divide the amount of heat required in the reaction by the amount of moles to find the enthalpy.
21.2kJ/0.487 mol=43.5 kJ/mol

Hope this helps!

Kayla Ikemiya 1E
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

Re: 8.37

Postby Kayla Ikemiya 1E » Tue Jan 16, 2018 2:11 pm

nevermind I understand now

Kayla Ikemiya 1E
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

Re: 8.37

Postby Kayla Ikemiya 1E » Tue Jan 16, 2018 2:12 pm

Shoot just saw this. Thank you Kelly!


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