At constant volume, the heat of combustion of a particular compound is –3947.0 kJ/mol. When 1.311 g of this compound (molar mass = 136.58 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 4.343 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

How much heat was generated.

3947.0 kJ/mol x (1.311/16.59) = q

Then q = Ccal*delta T
Substitute and solve for Ccal.

To determine the heat capacity of the calorimeter, we can use the formula:

q = C * ΔT

where:
q is the heat absorbed or released by the system
C is the heat capacity of the calorimeter
ΔT is the change in temperature of the calorimeter

First, let's convert the mass of the compound burned into moles:

moles = mass / molar mass
moles = 1.311 g / 136.58 g/mol

Next, we can use the heat of combustion to find the heat released during the reaction:

q = moles * heat of combustion
q = (1.311 g / 136.58 g/mol) * (-3947.0 kJ/mol)

Now, we need to convert the heat released to calories:

1 kJ = 1000 cal, so
q = (1.311 g / 136.58 g/mol) * (-3947.0 kJ/mol) * 1000 cal/kJ

Finally, we can use the formula to find the heat capacity:

C = q / ΔT

Plug in the values we have calculated to get the heat capacity of the calorimeter.