Problem: When a 3.80-g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.1 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.21 kJ/°C. Determine ΔE for octane combustion in units of kJ/mol octane.

FREE Expert Solution

Step 1

Q = CcalTQ = (6.21 kJ°C)(27.1°C)

Q = 168.291 kJ


Step 2

3.80 g C8H8 ×1 mol C8H8104.144 g C8H8 = 0.0365 mol C8H8


79% (96 ratings)
View Complete Written Solution
Problem Details

When a 3.80-g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.1 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.21 kJ/°C. Determine ΔE for octane combustion in units of kJ/mol octane.

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 Constant-Volume Calorimetry concept. You can view video lessons to learn Constant-Volume Calorimetry. Or if you need more Constant-Volume Calorimetry practice, you can also practice Constant-Volume Calorimetry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Sumner's class at UF.