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jbritlyn jbritlyn
wrote...
Posts: 5
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8 years ago
I'm trying to understand how to calculate the molar heat of combustion of a substance, given the heat capacity of a calorimeter as well as the mass of water that the calorimeter contains.
I cannot find any such problems online, and my book is of very little help.

Here is the example I am currently working on, and need help with:

10 g of methane (CH4) is combusted in a calorimeter that has an empty heat capacity of 18 J/°C.
The calorimeter contained 150 g of water. If the temperature changed from 25.2 °C to 30.3 °C,
calculate the molar heat of combustion of methane in J/mol.

The answer is given to me, which is -5270 J/mol. However, I am completely lost as to how I would arrive at that answer.
Please, please help!
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wrote...
Staff Member
Educator
8 years ago
Hope this helps:
Attached file
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Mastering in Nutritional Biology
Tralalalala Slight Smile
wrote...
8 years ago
[(4.18 J/gC) * 150 g H2O * 5.1 C] / (10 g CH4 / MW CH4 g/mole) =319.77
wrote...
2 years ago
Thank you
wrote...
A year ago
ty
Answer rejected by topic starter
wrote...
A year ago
The pdf is just the questions again lmao
wrote...
Staff Member
Educator
A year ago
The pdf is just the questions again lmao

Answers are at the very end of the document Undecided
Mastering in Nutritional Biology
Tralalalala Slight Smile
Anonymous
wrote...
2 months ago Edited: 2 months ago, Thomas vo
TY :)
wrote...
2 months ago
Thx
wrote...
2 months ago
Thanks
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