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?
Question:
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.
Answer:
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
So tell us your problem. What is it you don't understand.
Is it okay to have a negative temperature (in degrees Celsius) in this case?
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.
But I got an answer of 42.5K, which means when I convert it to degrees Celsius I get 42.5K - 273 K = -23.05 degrees Celsius.
Does this sound weird to you then?
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.
Oh, I see now. I really appreciate your help :) Have a wonderful day!
To calculate the increase in temperature of the calorimeter, you need to use the formula:
ΔT = (mass of CH4 * ΔEcombustion) / heat capacity
First, convert the mass of CH4 from grams to moles. Since the molar mass of CH4 is 16 g/mol, divide 67.2 g by 16 g/mol to get 4.20 mol.
Next, multiply the number of moles of CH4 by the ΔEcombustion value of -885.4 kJ/mol to find the heat released during combustion.
Now, divide the heat released by the heat capacity of the calorimeter, which is 87.5 kJ/K, to find the increase in temperature.
Alternatively, you can combine the previous steps into a single formula:
ΔT = (mass of CH4 * ΔEcombustion) / (molar mass of CH4 * heat capacity)
By substituting in the given values, you will be able to calculate ΔT, which is the increase in temperature of the calorimeter.