C3H6O + 4O2 --> 3CO2(g) + 3H2O(g) deltaH= -1790kJ

the density of C3H6O is 0.79g/mL. HOw much heat is released by the combustion of 150mL of acetone?

grams acetone = volume x density = approx 115 grams but you need a more accurate number than that.

So you get 1790 kJ for 58 g C3H6O; how much will you get from 115 g.

1790 x (115/58) = ? kJ released.

To find out how much heat is released by the combustion of 150mL of acetone (C3H6O), you can follow these steps:

Step 1: Calculate the mass of acetone (C3H6O) in grams.
Density is given as 0.79 g/mL. Therefore, the mass of 150 mL of acetone can be found by multiplying the volume (150 mL) by the density (0.79 g/mL):

Mass of acetone = 150 mL * 0.79 g/mL = 118.5 g

Step 2: Use the balanced equation to determine the mole ratio between C3H6O (acetone) and deltaH (heat of combustion).
From the balanced equation, it is indicated that 1 mole of acetone (C3H6O) releases -1790 kJ of heat in the combustion process.

Step 3: Convert the mass of acetone (in grams) to moles.
To convert mass to moles, you need to divide the mass of acetone by its molar mass. The molar mass of C3H6O can be calculated as follows:

Molar mass of C3H6O = (3 * molar mass of C) + (6 * molar mass of H) + (1 * molar mass of O)
= (3 * 12.01 g/mol) + (6 * 1.01 g/mol) + (1 * 16.00 g/mol)
= 38.03 g/mol + 6.06 g/mol + 16.00 g/mol
= 60.09 g/mol

Now, divide the mass of acetone (118.5 g) by its molar mass (60.09 g/mol):

Moles of acetone = 118.5 g / 60.09 g/mol ≈ 1.97 mol

Step 4: Calculate the amount of heat released by multiplying the moles of acetone by the heat of combustion per mole.
From the balanced equation, it is stated that the combustion of 1 mole of acetone releases 1790 kJ of heat.

Heat released = 1.97 mol * -1790 kJ/mol
≈ -3526.3 kJ

So, the combustion of 150 mL of acetone (C3H6O) will release approximately -3526.3 kJ of heat.

To calculate the amount of heat released by the combustion of acetone (C3H6O) in 150 mL, we can follow these steps:

Step 1: Calculate the mass of acetone in 150 mL.
Since the density of acetone is given as 0.79 g/mL, we can use this information to determine the mass of acetone in 150 mL.

Mass = Volume × Density
Mass = 150 mL × 0.79 g/mL

Step 2: Calculate the moles of acetone.
To do this, we need to know the molar mass of acetone, which is the sum of the atomic masses of its constituent elements.

Molar mass of C3H6O = (3 × molar mass of C) + (6 × molar mass of H) + (1 × molar mass of O)

You can find the atomic masses of carbon (C), hydrogen (H), and oxygen (O) on the periodic table. Add them up to get the molar mass of acetone.

Step 3: Use the balanced equation to determine the moles of CO2 produced.
From the balanced equation, we can see that 1 mole of acetone (C3H6O) produces 3 moles of CO2 (carbon dioxide).

Step 4: Calculate the heat released.
The given value of deltaH (change in heat) is -1790 kJ for the combustion of 1 mole of acetone.

We have the moles of acetone from Step 2, and we know that 1 mole of acetone releases -1790 kJ (negative sign indicates the release of heat). Therefore, we can calculate the total heat release using the following formula:

Heat release = deltaH × moles of acetone

Remember to pay attention to the units of moles and deltaH so that they are consistent for the calculation.

By following these steps, you can calculate the exact amount of heat released by the combustion of 150 mL of acetone.