Question

The heat of combustion of ethanol, C₂H₅OH, is 29.52 kJ/g. Combustion of 5.99 g of - ethanol causes a temperature rise of 1.77 °C in a certain bomb calorimeter. What is the heat capacity of this bomb calorimeter?

Answer 1

Using the provided heat of combustion for ethanol and the observed temperature change in the bomb calorimeter, the heat capacity is determined to be 100.0 kJ/°C by dividing the total heat released by the change in temperature.

Step-by-step explanation:

The heat of combustion of ethanol (C₂H₅OH) can be used to determine the heat capacity of the bomb calorimeter. Heat capacity (C) is calculated by the formula C = q/ΔT, where q is the heat absorbed or released, and ΔT is the change in temperature. Here, we have 5.99 g of ethanol and ΔT is 1.77°C. Given the heat of combustion is 29.52 kJ/g, we first calculate the total heat released:

• q = mass of ethanol (g) × heat of combustion (kJ/g) = 5.99 g × 29.52 kJ/g = 176.89 kJ.

Now we calculate the heat capacity of the bomb calorimeter:

• C = q/ΔT = 176.89 kJ / 1.77°C = 100.0 kJ/°C.

Therefore, the heat capacity of the bomb calorimeter is 100.0 kJ/°C.