Final answer:
To find the number of calcium atoms in 1.00 g, we calculate the number of moles of calcium and then multiply by Avogadro's number, resulting in approximately 1.50×1022 calcium atoms.
Step-by-step explanation:
The number of calcium atoms in 1.00 g can be determined by first finding the molar mass of calcium, which is approximately 40.08 g/mol. Next, we calculate the number of moles in 1.00 g using the formula number of moles = mass (g) / molar mass (g/mol). Then, to find the number of atoms, we multiply the number of moles by Avogadro's number, which is approximately 6.022×1023 atoms/mol.
To illustrate, here are the calculations:
- Calculate the number of moles of calcium in 1.00 g: (1.00 g) / (40.08 g/mol) = 0.02495 mol
- Calculate the number of atoms of calcium: (0.02495 mol) × (6.022×1023 atoms/mol) = 1.50×1022 atoms
Therefore, there are approximately 1.50×1022 calcium atoms in 1.00 g of calcium.
In order to determine the number of atoms of calcium in 1.00 g, we need to use the concept of molar mass and Avogadro's number. The molar mass of calcium is 40.08 g/mol. Using this information, we can calculate the number of moles of calcium in 1.00 g by dividing the mass by the molar mass:
Number of moles = Mass / Molar mass = 1.00 g / 40.08 g/mol = 0.0249 mol
Now, since 1 mole of any substance contains Avogadro's number of particles (6.022 x 10^23), we can calculate the number of atoms:
Number of atoms = Number of moles x Avogadro's number = 0.0249 mol x 6.022 x 10^23 atoms/mol = 1.50 x 10^22 atoms