Heat Capacity and CalorimetryHomework Answers
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25C to 33.73C.
If the heat capacity of the calorimeter and contents is 9.63kJ/C,
what is the value of q for burning 1.00 lol of ethanol at constant volume and 25.00C.
Is q equal to U or H?
formula
q calorimeter = C x ΔT
where,
C = heat capacity = 9.63 kJ/ºC
ΔT = (Tf-Ti) = 33.73ºC - 25ºC = 8.73ºC
So,
q calorimeter = (9.63 kJ/ºC) x (8.73ºC) = + 84.0699 kJ
q reaction = - q calorimeter
q reaction = - 84.0699 kJ
================================
"q for burning 1 mol of ethanol",
mol C2H5OH =
(2.84g C2H5OH) x (1mol C2H5OH/46.068g C2H5OH)
= 0.061648 mol C2H5OH
Now, q reaction / mol = (84.0699 kJ / 0.061648 mol)
= -1,363.71 kJ/mol C2H5OH
--------------------------------------...
What is the value of q for burning 1 mol of ethanol?
q = (1 mol C2H5OH) x (-1,363.71 kJ/mol C2H5OH)
= -1,363.71 kJ = -1.36371 x 10^3 kJ
= -1.36 x 10^3 kJ ---------------answer
=============================================
not equal
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