Consider the following thermochemical equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover:
C3C6O + 4 O2 --> 3 CO2 + 3H2O
DELTA Hrxm= -1790kJ
If a bottle of nail polish remover contains 183 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL.
grams acetone = volume x density = ?
1790 x (grams acetone/molar mass acetone) = ?
so 1790 x (183/58.08) ?
No. You don't have 183 g acetone do you? That's 183 mL acetone, not grams.
You must use the density to convert 183 mL to grams.
To calculate the amount of heat released by the complete combustion of acetone, we need to follow these steps:
Step 1: Convert the volume of acetone from milliliters (mL) to grams (g).
Given that the density of acetone is 0.788 g/mL and the volume is 183 mL, we can use the following conversion:
Volume (mL) x Density (g/mL) = Mass (g)
183 mL x 0.788 g/mL = 144.204 g
So, the mass of acetone is approximately 144.204 g.
Step 2: Calculate the amount of heat released using the molar ratio and the enthalpy change.
From the balanced thermochemical equation, we know that the molar ratio between acetone and the enthalpy change is 1:1. This means that for every 1 mole of acetone combusted (-1790 kJ) is released.
To calculate the amount of heat released, we need to determine the number of moles of acetone present. To do this, we'll need to find the molar mass of acetone.
The molar mass of C3H6O is:
3(12.01 g/mol) + 6(1.01 g/mol) + 16.00 g/mol = 58.08 g/mol
Now, we can use the molar mass to convert grams of acetone to moles:
Mass (g) / Molar Mass (g/mol) = Moles (mol)
144.204 g / 58.08 g/mol ≈ 2.483 mol
Since the molar ratio between acetone and the enthalpy change is 1:1, the amount of heat released is:
2.483 mol x (-1790 kJ/mol) = -4447.57 kJ
Therefore, approximately -4447.57 kJ of heat would be released by the complete combustion of the 183 mL bottle of nail polish remover.