How Many Carbon Atoms in 15.6 kg of Acetone?
Calculating the Number of Carbon Atoms in 15.6 kg of Acetone
Acetone is represented by the chemical formula CH3COCH3. The density of acetone is 1.30 g/ml.
To calculate the number of carbon atoms in 15.6 kg of acetone, we can follow these steps:
Step 1:First, convert the mass of acetone from kilograms to grams:
15.6 kg = 15.6 kg * 1000 g/kg = 15600 g
Step 2:Next, calculate the number of moles of acetone present:
n(CH3COCH3) = m(CH3COCH3) ÷ M(CH3COCH3)
n(CH3COCH3) = 15600 g ÷ 58 g/mol
n(CH3COCH3) = 268.965 mol
Step 3:Calculate the total number of acetone molecules:
N(CH3COCH3) = n(CH3COCH3) * Avogadro's number
N(CH3COCH3) = 268.965 mol * 6.022 * 10^23 1/mol
N(CH3COCH3) = 1.619 * 10^26
Step 4:Since there are three carbon atoms in one molecule of acetone, calculate the total number of carbon atoms:
n(C) = 3 * 1.619 * 10^26 = 4.859 * 10^26
Therefore, there are 4,859·10²⁶ atoms of carbon in 15.6 kg of acetone.
How many moles of acetone are present in 15.6 kg of acetone? 15.6 kg is equivalent to 15600 g. The molar mass of acetone is 58 g/mol. Therefore, 15600/58 = 269 moles. 1 mole of acetone contains 3 * 6.022 * 10^23 atoms. Therefore, 269 moles of acetone would contain: 269 * 3 * 6.022 * 10^23 atoms = 4.86 * 10^26 atoms of carbon.