Posted by Anne on Wednesday, December 12, 2007 at 8:26pm.
drwls, if you are there, I got an answer of 42.5 Kelvin, so then that means it is a negative number if converted to degrees Celsius?
The heat capacity of a bomb calorimeter is 87.5 kJ/K (this value is for the total heat capacity including that of the water jacket around the reaction chamber). If 67.2g of CH4 (g), is combusted under such reaction conditions, what will be the increase in temperature of the calorimeter? Delta Ecombustion for CH4 (g) is -885.4 kJ/mol.
drwls, Wednesday, December 12, 2007 at 7:38am
Calculate the heat energy release:
The number of moles of CH4 you are burning is 67.2/16 = 4.20 mol
Multiply that by 885.4 kJ/mol for the heat release. Then divide that by 87.5 kJ/K for the temperature rise.
Or, you could do it all at once
Delta T = (67.2g*885.4kJ/mol)/(16 g/mol*87.5 kJ/K) = ? K
Chemistry - DrBob222, Wednesday, December 12, 2007 at 8:43pm
So tell us your problem. What is it you don't understand.
Chemistry - Anne, Wednesday, December 12, 2007 at 9:01pm
Is it okay to have a negative temperature (in degrees Celsius) in this case?
Chemistry - DrBob222, Wednesday, December 12, 2007 at 9:08pm
Combustion reactions give off energy, as this one does; therefore, the temperature will rise. The question asks for how much the T will rise. So, no, I wouldn't expect the T to go down.
Chemistry - DrBob222, Wednesday, December 12, 2007 at 9:29pm
Yes, it's weird. But your answer is correct; you're just confused on what your answer is. I worked the problem and I have 42.5 degrees BUT THAT IS DELTA T. That IS the rise in degrees C or degrees K (both are equivalent). The problem didn't ask for the T, it asked for delta T and that is what the equation is.
delta H = delta E = Cp*delta T
885.4 kJ/mol* 4.2 mol = 87.5 kJ*delta T.
Solve for delta T = 42.5 degrees K (or 42.5 degrees C.).
Glad I could help.
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