At constant volume, the heat of combustion of a particular compound is –3547.0 kJ/mol. When 1.239 g of this compound (molar mass = 196.58 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.539 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

q = heat combustion

q = heat capacity x delta T
q = Cp x 8.539
delta H = 3547.0 kJ/mol so
q = 3547.0 kJ x (1.239/196.58) = ?
Substitute and solve for Cp.

To find the heat capacity (calorimeter constant) of the calorimeter, we can use the equation Q = m × C × ΔT, where Q is the heat absorbed or released, m is the mass of the substance, C is the heat capacity, and ΔT is the change in temperature.

In this case, we have the following information:
- Heat of combustion (Q) = –3547.0 kJ/mol (negative sign indicates heat released)
- Mass of compound (m) = 1.239 g
- Molar mass of the compound = 196.58 g/mol
- Change in temperature (ΔT) = 8.539 °C

First, we need to calculate the moles of the compound burned:
moles = mass / molar mass
moles = 1.239 g / 196.58 g/mol
moles ≈ 0.0063 mol

Next, we can find the amount of heat released (Q) in kJ:
Q = –3547.0 kJ/mol × 0.0063 mol
Q ≈ –22.37 kJ

Now, we can use the equation Q = m × C × ΔT to find the heat capacity (C) of the calorimeter:
C = Q / (m × ΔT)
C = –22.37 kJ / (1.239 g × 8.539 °C)
C ≈ –22.37 kJ / (10.6 g·°C)
C ≈ –2.11 kJ/g·°C

The heat capacity of the calorimeter is approximately –2.11 kJ/g·°C. The negative sign indicates that the calorimeter releases heat instead of absorbing it.