🤓 Based on our data, we think this question is relevant for Professor Marinescu's class at USC.
At constant pressure, q = ΔH
produce heat → (-) q
q = - 2658 kJ
Lighters are usually fueled by butane (C4H10). When 1 mole of butane burns at constant pressure, it produces 2658 kJ of heat and does 3 kJ of work. What is the value of ΔH for the combustion of one mole of butane?
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 Internal Energy concept. You can view video lessons to learn Internal Energy. Or if you need more Internal Energy practice, you can also practice Internal Energy practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Marinescu's class at USC.