Well, the question is what part of a mole of acetone do you have?
get the mass from volume and density, then divide that mass by molmass.
consider the following thermochemical equation for the combustion of acetone
C3H6O(l)+4O2(g)---->3CO2(g)+3H2O(g)
delta H rxn=-1790kJ.
If a bottle of nail polish remover contains 179mL of acetone, how much heat would be released by its complete combustion? the density of acetone is .788g/mL. answer in kJ
2 answers
1212