Fingernail polish is mainly acetone (C3H6O) and has a density of 0.788gcc.
A. HOW MANY GRAMS OF ACETONE ARE IN A O.5L BOTTLE
B HOW MANY MOLECULES OF ACETONE ARE IN THAT SAME BOTTLE
You made a typo. You meant the density is 0.789 g/cc.
A.
mass = volume x density
mass = 500 cc x 0.789 g/cc = ?
B. mols acetone = grams/molar mass
Then there are 6.02E23 molecules in one (1) mol of acetone.
To calculate the grams of acetone in a 0.5L bottle and the number of molecules of acetone in the bottle, we'll follow these steps:
Step 1: Calculate the mass of acetone in grams.
Step 2: Convert the mass of acetone into the number of moles.
Step 3: Calculate the number of molecules using Avogadro's number.
Step 1: Calculate the mass of acetone in grams.
Density is defined as mass (g) per unit volume (cc or mL). In this case, the density of acetone is given as 0.788 g/cc. Since 1 cc is equal to 1 mL, we can directly use 0.788 g/mL.
Mass = Density x Volume
Mass = 0.788 g/mL x 500 mL
Mass = 394 g
Therefore, there are 394 grams of acetone in a 0.5L bottle.
Step 2: Convert the mass of acetone into the number of moles.
The molar mass of acetone (C3H6O) can be calculated by adding up the atomic masses of carbon, hydrogen, and oxygen:
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of O = 16.00 g/mol
Molar mass of acetone (C3H6O) = (3 x 12.01) + (6 x 1.01) + 16.00 = 58.08 g/mol
Number of moles = Mass / Molar mass
Number of moles = 394 g / 58.08 g/mol
Number of moles = 6.78 moles
Therefore, there are approximately 6.78 moles of acetone in the bottle.
Step 3: Calculate the number of molecules using Avogadro's number.
Avogadro's number (NA) is the number of particles (atoms, molecules, etc.) in one mole of a substance, approximately equal to 6.022 x 10^23.
Number of molecules = Number of moles x Avogadro's number
Number of molecules = 6.78 moles x 6.022 x 10^23 molecules/mol
Number of molecules ≈ 4.085 x 10^24 molecules
Therefore, there are approximately 4.085 x 10^24 molecules of acetone in the 0.5L bottle.