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Question

Need Help!! Will give reward for first right answer!
Many cigarette lighters contain liquid butane,C4H10(l). Using standard enthalpiesof formation, calculate the quantity of heat producedwhen1.8 g of butane is completely combusted inair under standard conditions

Answers

is -88.5 kJ

1. Find how many moles of butane in 1.8 grams usingstoichiometry. The molecular weight of butane can be foundusing the periodic table (C=12 andH=1 so 12x4 and Hx10)

1.8 g butane x 1 mol/58g butane

2. Then use the standard enthalpy of formation of butane(usually found in the appendix of chemistry books) to find the heatproduced.

1.8 g butane x 1 mol/58 gbutanex -126.15 kJ/mol

grams of butane cancel out, and mol of butane cancel out and youare left in kJ of heat generated from the reaction


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