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 0.788g/ml
You need to know the heat of combustion (kJ/mol) or heat of reaction.
To calculate the amount of heat released by the complete combustion of acetone, we need to determine the amount of acetone in grams.
To do this, we can use the density of acetone. The formula for density is:
Density = Mass / Volume
Rearranging the formula, we find:
Mass = Density x Volume
Given that the density of acetone is 0.788 g/ml and the volume of acetone is 176 mL, we can calculate the mass of acetone:
Mass = 0.788 g/ml x 176 ml = 138.688 g
Now, we will use the molar mass of acetone to convert the mass of acetone to moles. The molar mass of acetone is 58.08 g/mol.
Moles = Mass / Molar mass
Moles = 138.688 g / 58.08 g/mol = 2.39 mol
Next, we will use the balanced chemical equation for the combustion of acetone to determine the heat released per mole of acetone. The balanced equation is:
C3H6O + 4O2 → 3CO2 + 3H2O
From the equation, we can see that for the complete combustion of one mole of acetone, three moles of carbon dioxide (CO2) are produced. According to the standard enthalpy of combustion, the combustion of one mole of acetone releases 1790 kJ of heat.
Therefore, the amount of heat released by the complete combustion of 2.39 moles of acetone can be calculated as follows:
Heat released = Moles of acetone x Heat released per mole
Heat released = 2.39 mol x 1790 kJ/mol = 4282.1 kJ
Therefore, the heat released by the complete combustion of the acetone in the bottle of nail polish remover would be approximately 4282.1 kJ.