Question

2025 Consider the following themochemical equation for the corbution of acetone (C,H,O), the main ingredient in na polish remover C104) + 4 0 (g) + 30 (9) + 3H00 9) AH-1790 kJ Part A a bottle of nail polish remover contain 178 ml of acetone, how much hat would be released by its complete combustion? The density of acetone is 0788 / mL AH- Subm Provide Feedback Nex

Answer 1

C3H6O + 4O2---> 3CO2 + 3H2O

Here given that = Volume of the Accetone = 178mL

density = 0.788g/mL

So mass of the Substance = 178*0.788= 140.26g

Molecular mass of Accetone = 58g

Mole of the Accetone = 140.26/58 = 2.41 mol

Here given that delH for 1mole of Accetone = -1790 Kj

So the Heat of combustion for 2.41 mole of Accetone = 2.41 * (-1790) = -4313.9 Kj

Negetive sign reffered to the release of the heat / Energy

If we take the quantity of Heat = 4313.9 Kj

Thank you

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