Question

At constant volume, the heat of combustion of a particular compound is -3068.0 kj/mol. when 1.717g of this compound (molar mass = 115.09 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 7.257 c. what is the heat capacity (calorimeter constant) of the calorimeter? )

Answer 1

The heat capacity of the calorimeter is calculated using the heat released by the combustion of a compound and the temperature change of the calorimeter. The total heat released is first found by multiplying the heat of combustion by the number of moles combusted. Then, the calorimeter constant is found by dividing the heat released by the temperature change.

Step-by-step explanation:

To find the heat capacity of the calorimeter, we first need to calculate the amount of heat (q) released by the combustion of the compound. Using the data provided, the heat of combustion is -3068.0 kJ/mol, and the mass of the compound burned is 1.717 g. First, we calculate the number of moles of the compound burned:

• Number of moles = 1.717 g / 115.09 g/mol = 0.01492 mol
• Total heat released = -3068.0 kJ/mol × 0.01492 mol = -45.78096 kJ

To find the calorimeter constant (C), use the formula q = C × ΔT, where q is the heat released and ΔT is the temperature change. Rearranging the formula gives us C = q / ΔT. Now we can plug in the heat released and the temperature change:

• Calorimeter constant (C) = -45.78096 kJ / 7.257 °C = -6.311 kJ/°C