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?
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