Question

Consider the following equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover.

C3H6O(l) + 4O2(g) → 3CO2(g) + 3H2O(g) ΔHrxn = −1790kJ
If a bottle of nail polish remover contains 143 g of acetone, how much heat would be released by its complete combustion? Express your answer to three significant figures.

Answer 1

Molar mass of Acetone

• C3H6O
• 3(12)+6+16
• 58g/mol

Now

• 1 mol releases -1790KJ heat .

Moles of Acetone:-

• 143/58=2.5mol

Amount of heat:-

• 2.5(-1790)=-4475kJ