Themoonlight
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#1
Report Thread starter 1 month ago
#1
This might seem like an easy question but I’m really stuck on it:

Why is the heat change calculated from a bomb calorimeter not an enthalpy change?

Any answers/ explanations would be much appreciated
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Hellllpppp
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I can think of two possible routes to go with this question
1) you can not calculate heat change accurately - think about why
2) think about the units
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Pyruvic Acid
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As above. Also, enthalpy change is simply heat change measured at a constant pressure. Perhaps we can't measure enthalpy change using bomb calorimeter because the pressure does not usually stay constant during the experiment?
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scimus63
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isn't it just an enthalpy change! Its just measuring the heat produced by combustion!
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Themoonlight
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(Original post by Hellllpppp)
I can think of two possible routes to go with this question
1) you can not calculate heat change accurately - think about why
2) think about the units
Thank you!
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Themoonlight
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#6
Report Thread starter 4 weeks ago
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(Original post by Pyruvic Acid)
As above. Also, enthalpy change is simply heat change measured at a constant pressure. Perhaps we can't measure enthalpy change using bomb calorimeter because the pressure does not usually stay constant during the experiment?
Ah okay, this makes sense. Thank you.
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Themoonlight
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#7
Report Thread starter 4 weeks ago
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(Original post by scimus63)
isn't it just an enthalpy change! Its just measuring the heat produced by combustion!
That’s what I thought but I’ve seen a lot of suggestions regarding the fact that pressure doesn’t always remain constant so I feel as though this plays into it.
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