If a bottle of nail polish remover contains 176 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL.

Question

Consider the following thermochemical equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover.
C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g)ΔH∘rxn=−1790kJ

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Answer 1 · 2018-01-04T19:10:50

Approx...#-4000*kJ#

We gots the combustion reaction....

#"H"_3"CC(=O)CH"_3"(l)" + "4O"_2"(g)" rarr "3CO"_2"(g)+3H"_2"O(l)"+Delta#

#"Moles of acetone"=(176*mLxx0.788*g*mL^-1)/(58.08*g*mol^-1)=2.39*mol#

We are given that #DeltaH_"combustion"^@=-1790*kJ*mol^-1#...were #mol^-1# means #"per mole of reaction as written..."#...

And so we take the product....

#-1790*kJ*mol^-1xx2.39*mol=??kJ#