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Topic: Enthalpy/Thermochemical Stoichiometry  (Read 12712 times)

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Offline viet

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Enthalpy/Thermochemical Stoichiometry
« on: October 14, 2008, 11:03:38 AM »
Quote
Consider the following thermochemical equation for the combustion of acetone C3H6O the main ingredient in nail polish remover.
C3H6O (l) + 4O2 (g) => 3CO2 (g) + 3H2O (g)    /\Hrxn = -1790 kJ

If a bottle of nail polish remover contains 176 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL.

|/\H| = ?

i tried solving this by doing:
176mL (0.788g/mL) = 138.688g

138.688g C3H6O (1 mol C3H6O / 58.081g C3H6O) (-1790kJ / 1 mol C3H6O) = -4507.026 kJ

the answer i got is wrong, can someone help?

Offline Astrokel

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Re: Enthalpy/Thermochemical Stoichiometry
« Reply #1 on: October 14, 2008, 11:21:23 AM »
hey viet,

Quote
138.688g C3H6O (1 mol C3H6O / 58.081g C3H6O) (-1790kJ / 1 mol C3H6O) = -4507.026 kJ
i got a different value from your working..
No matters what results are waiting for us, it's nothing but the DESTINY!!!!!!!!!!!!

Offline viet

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Re: Enthalpy/Thermochemical Stoichiometry
« Reply #2 on: October 14, 2008, 12:51:18 PM »
thanks for replying Astrokel, i seem to did the calculation wrong. thanks  :D

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