Lighters are usually fueled by butane (C4H10). When 1 mole of butane burns at constant pressure it produces 2658kJ of heat and does 3kJ of w?

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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 are the values of ΔH and ΔE for the combustion of one mole of butane?Could you please explain this

Dr. Summer Schneider PhD · Accepted Answer

So, consider the necessary formulas:deltaH = q - PdeltaVdeltaE = q + wFirst, to find delta E:The reaction PRODUCES 2658 kJ of h (q), and does 3 kJ of work (w).2658 kJ(q) + 3 kJ(w) = 2661 kJ, BUT the reaction PRODUCES heat, which means deltaE is negative.deltaE = -2661Second, to find deltaH:deltaH = q - PdeltaVdeltaH = 2658 kJ(q) - PdeltaVNow, the question states that butane burns at a constant pressure; that just translates to the pressure of the reaction is equal to 0.deltaH = 2658 kJ(q) - (0)deltaVdeltaH = 2658 kJ(q) - 0deltaH = 2658 kJ, BUT, like before, the reaction PRODUCES heat, which also mean deltaH is negative.deltaH = -2658 kJI hope this helped! Have a nice week.

Ms. Mara Collier

Lighters are usually fueled by butane (C4H10). When 1 mole of butane burns at constant pressure it produces 2658kJ of heat and does 3kJ of w?

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