Calculate the number of carbon atoms in 0.75 L of acetone (CH3COCH3). (density=1.3g/mL and boiling point=48.5 degrees)

To calculate the number of carbon atoms in a given volume of acetone, we need to follow a series of steps:

Step 1: Determine the mass of acetone.
Given the density of acetone, which is 1.3 g/mL, and the volume, which is 0.75 L, we can use the density formula to find the mass.
Mass = density × volume
Mass = 1.3 g/mL × 0.75 L = 0.975 g

Step 2: Calculate the number of moles of acetone.
To find the number of moles, we need to divide the mass of acetone by its molar mass. The molar mass of acetone can be calculated by adding up the individual atomic masses of its components.
Molar mass of acetone (CH3COCH3):
(12.01 g/mol × 3) + (1.01 g/mol × 6) + (16.00 g/mol × 1) = 58.08 g/mol

Number of moles = Mass / Molar mass
Number of moles = 0.975 g / 58.08 g/mol ≈ 0.0168 mol

Step 3: Calculate the number of carbon atoms.
One mole of a substance contains 6.022 × 10^23 particles. This is known as Avogadro's number.
Number of carbon atoms = Number of moles × Avogadro's number
Number of carbon atoms = 0.0168 mol × 6.022 × 10^23 atoms/mol ≈ 1.01 × 10^22 atoms

Therefore, there are approximately 1.01 × 10^22 carbon atoms in 0.75 L of acetone.