[viet]

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)    /\H_rxn = -1790 kJ

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.

|/\H| = ?

i tried solving this by doing:
176mL (0.788g/mL) = 138.688g

138.688g C₃H₆O (1 mol C₃H₆O / 58.081g C₃H₆O) (-1790kJ / 1 mol C₃H₆O) = -4507.026 kJ

the answer i got is wrong, can someone help?

[Astrokel]

hey viet,

138.688g C3H6O (1 mol C3H6O / 58.081g C3H6O) (-1790kJ / 1 mol C3H6O) = -4507.026 kJ

i got a different value from your working..

[viet]

thanks for replying Astrokel, i seem to did the calculation wrong. thanks