consider the following thermochemical equation for the combustion of acetone

C3H6O(l)+4O2(g)---->3CO2(g)+3H2O(g)
delta H rxn=-1790kJ.

If a bottle of nail polish remover contains 179mL of acetone, how much heat would be released by its complete combustion? the density of acetone is .788g/mL. answer in kJ

Well, the question is what part of a mole of acetone do you have?

get the mass from volume and density, then divide that mass by molmass.

To find out how much heat would be released by the complete combustion of the acetone in the nail polish remover, we need to calculate the moles of acetone using the given volume and density, and then use the molar ratio from the balanced thermochemical equation to determine the amount of heat released.

First, let's determine the mass of acetone in the bottle of nail polish remover:
Mass = Volume x Density
Mass = 179 mL x 0.788 g/mL = 141.052 g

Next, let's calculate the moles of acetone:
Moles = Mass / Molecular Weight
The molecular weight of acetone (C3H6O) is:
(3 x atomic weight of Carbon) + (6 x atomic weight of Hydrogen) + (1 x atomic weight of Oxygen) = (3 x 12.01 g/mol) + (6 x 1.01 g/mol) + (1 x 16.00 g/mol) = 58.08 g/mol

Moles = 141.052 g / 58.08 g/mol = 2.43 mol (approximately)

Now we can use the molar ratio from the balanced equation to calculate the amount of heat released:
According to the thermochemical equation, the molar ratio between acetone and heat released is 3:1790 kJ.

Heat released = Moles of acetone x Delta H
Heat released = 2.43 mol x (-1790 kJ/3 mol)
Heat released ≈ -3063.3 kJ

Therefore, approximately -3063.3 kJ of heat would be released by the complete combustion of the 179 mL nail polish remover bottle containing acetone.

To find the amount of heat released by the complete combustion of acetone, we need to calculate the moles of acetone present in the given volume and then use the molar ratio from the balanced equation to find the heat released.

Here are the steps to find the answer:

Step 1: Calculate the mass of acetone.
Given that the density of acetone is 0.788 g/mL and the volume is 179 mL, we can find the mass using the formula:
Mass = Volume x Density
Mass = 179 mL x 0.788 g/mL
Mass = 141.052 g

Step 2: Convert mass to moles.
Using the molar mass of acetone, we can convert the mass to moles:
Molar mass of acetone (C3H6O) = 12.01 g/mol (C) + 1.01 g/mol (H) x 6 + 16.00 g/mol (O)
Molar mass of acetone = 58.08 g/mol

Moles of acetone = Mass / Molar mass
Moles of acetone = 141.052 g / 58.08 g/mol
Moles of acetone ≈ 2.4289 mol

Step 3: Calculate the heat released.
According to the balanced equation, the molar ratio between acetone and the released heat is 1:1790 kJ.
Therefore, the heat released can be calculated using the following formula:
Heat released = Moles of acetone x ΔHrxn (per mole)
Heat released ≈ 2.4289 mol x (-1790 kJ/mol)
Heat released ≈ -4347.213 kJ

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

Therefore, the amount of heat released by the complete combustion of the nail polish remover containing 179 mL of acetone is approximately 4347.213 kJ.

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