Question
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
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
Answers
bobpursley
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.
get the mass from volume and density, then divide that mass by molmass.
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