4. If you were asked to determine the number of atoms in a 52.0 gram sample of carbon, how would you set up the conversion? What is the final answer with correct units?
mols C in 52.0g C is
mols = grams/atomic mass = 52/12 = ?
Then there are 6.022E23 atoms in 1 mols of atoms.
mols C in 52.0g C is
mols = grams/atomic mass = 52/12 = ?
Then there are 6.022E23 atoms in 1 mol of any kind.
To determine the number of atoms in a sample of carbon, you need to use the concept of molar mass and Avogadro's number. Here's how you can set up the conversion:
1. Start with the given mass of carbon: 52.0 grams.
2. Find the molar mass of carbon from the periodic table. The molar mass of carbon is approximately 12.01 grams/mol.
3. Use the molar mass to convert grams to moles by dividing the given mass by the molar mass:
52.0 g / 12.01 g/mol = 4.33 moles of carbon (rounded to two decimal places).
4. Avogadro's number, 6.022 x 10^23, represents the number of atoms in one mole of a substance.
5. Multiply the number of moles by Avogadro's number to find the number of atoms:
4.33 mol x 6.022 x 10^23 atoms/mol = 2.61 x 10^24 atoms (rounded to three significant figures).
So, the final answer is that there are approximately 2.61 x 10^24 atoms of carbon in a 52.0 gram sample.