Determine the heat involved during the combustion of anthracene using the calorimetry equation and the provided values
In bomb calorimetry, we can determine the heat of combustion by analyzing the temperature rise in water. In mathematical terms, the heat released by anthracene is equal to the heat absorbed by water:
We will use the heat released by the reaction to calculate its initial temperature. Recall that heat can be calculated using the following equation:
q = heat, J
When 0.455 g of anthracene, C14H10 (molar mass = 178.23 g/mol) is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g • °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.
A) -39.7 kJ/mol
B) -8120 kJ/mol
C) -7060 kJ/mol
D) +39.7 kJ/mol
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofWhen 0.455 g of anthracene, C14H10 (molar mass = 178.23 g/mo...as high difficulty.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Marin's class at UCF.