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If a bottle of nail polish remover contains 151 g of acetone, how much heat would be released by its complete combustion? ?
Consider the following equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover.
C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g)ΔHrxn=−1790kJ
1 Answer
- jacob sLv 72 months agoFavorite Answer
Solution :
The combustion of acetone is given as,
C3H6O + 4O2 = 3CO2 + 3H2O , ΔH = -1790 kJ
Number of moles in 151 g of acetone = Mass. /Molar mass
= 151 g / 58.08 g mol-1 = 2.59986 mol
Since, 1 mol of acetone produces 1790 kJ heat
Hence, 2.599 mol produces = 2.599 mol x 1790 kJ/1 mol
= 4653.75 kJ
Hence, heat released = 4653.75 kJ
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