If a bottle of nail polish remover contains 179 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 {\rm{g}}/{{\rm{mL}}}

The problem needs to be deciphered.

To calculate the amount of heat released by the complete combustion of acetone, we need to determine the mass of acetone and use its heat of combustion.

First, we'll calculate the mass of acetone in the bottle:

Mass = Volume x Density

Given:
Volume = 179 mL
Density = 0.788 g/mL

Mass = 179 mL x 0.788 g/mL
Mass = 141.452 g

Next, we need to know the heat of combustion of acetone. The heat of combustion is the amount of heat released when one mole of a substance undergoes complete combustion. The heat of combustion for acetone is typically given in kJ/mol.

The heat of combustion of acetone is approximately -1791 kJ/mol.

To convert grams of acetone to moles, we need to know the molar mass of acetone.

Molar Mass of Acetone (C₃H₆O) = (12.01 g/mol x 3) + (1.01 g/mol x 6) + (16.00 g/mol x 1)
Molar Mass of Acetone = 58.08 g/mol

Now, we can calculate the moles of acetone:

Moles = Mass / Molar Mass
Moles = 141.452 g / 58.08 g/mol
Moles ≈ 2.434 mol

Finally, we can calculate the amount of heat released by the complete combustion of acetone:

Heat Released = Moles x Heat of Combustion
Heat Released = 2.434 mol x -1791 kJ/mol
Heat Released ≈ -4362 kJ

Note: The negative sign indicates that heat is released during the combustion process.

Therefore, the amount of heat released by the complete combustion of the acetone in the nail polish remover would be approximately 4362 kJ.