Problem: 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?

🤓 Based on our data, we think this question is relevant for Professor Marinescu's class at USC.

FREE Expert Solution

At constant pressure, q = ΔH


produce heat  (-) q


q = - 2658 kJ 


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Problem Details

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?

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What professor is this problem relevant for?

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