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Topic: Constant volume calorimetry  (Read 4756 times)

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Offline imperius

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Constant volume calorimetry
« on: September 22, 2007, 01:55:05 PM »
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid. In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2820 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.40 °C. When a 0.2024-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.28 °C. What is the energy of combustion per unit mass of the unknown substance?

I have no idea how to do this problem
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Offline Bakegaku

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Re: Constant volume calorimetry
« Reply #1 on: September 22, 2007, 02:06:39 PM »
Do you have any equations that are related to enthalpy that you can think you can use?  How much energy was released by the salicylic acid to raise it 1.4ºC and how much energy would be needed to raise it 3.28ºC?
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Offline imperius

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Re: Constant volume calorimetry
« Reply #2 on: September 22, 2007, 02:15:25 PM »
the 3.28 Deg C was about an unknown substance. They are burned in the same calorimeter.

Equations: H = E + PV

s = q / (m*t)
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