mols compound = 1.489/131.02 = about 0.0114 but you need to do that more accurately.
kJ heat added to calorimeter = 3323 kJ/mol x 0.0114 mol = ? Then substitute this into
q = Ccal x delta T
Solve for Ccal.
At constant volume, the heat of combustion of a particular compound is –3323.0 kJ/mol. When 1.489 g of this compound (molar mass = 131.02 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.077 °C. What is the heat capacity (calorimeter constant) of the calorimeter?
1 answer
3 answers