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

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.
1212
Similar Questions
  1. C3H6O + 4O2 --> 3CO2(g) + 3H2O(g) deltaH= -1790kJthe density of C3H6O is 0.79g/mL. HOw much heat is released by the combustion
    1. answers icon 1 answer
    1. answers icon 3 answers
  2. given the thermochemical equations,B2O3 + 3H2O -> 3O2 + B2H6 delta h = -2035 kj H2O -> H2O delta h = 44 kj H2 + 1/2O2 -> H2O
    1. answers icon 1 answer
  3. Consider the combustion of propane:C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l) delta H= -2221 kJ Assume that all of the heat comes
    1. answers icon 3 answers
more similar questions