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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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Emajano Emajano
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7 years ago
When 1.820 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 34.52°C. Assuming that the specific heat of water is 4.18 J/(g ∙ °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.  Please explain step by step Slight Smile
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#1
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7 years ago
Q = 500.0 x 4.28 x 25.89 = 54110 J

moles C14H10 = 1.365 g /178.234 g/mol=0.007658

0.007658 : 54110 = 1 : x
x =7.06 x 10^6 J => 7060 = heat released by one mole

enthalpy = - 7060 kJ/mol
Emajano Author
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#2
7 years ago
where did the 4.28 come from? Face with Cold Sweat
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bolbolbolbol
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#3
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7 years ago
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