Final answer:
There are approximately 5.02 × 1022 atoms of carbon in 1.00 g of carbon, determined using the molar mass of carbon and Avogadro's number.
Step-by-step explanation:
To determine how many atoms of carbon are in 1.00 g of carbon, we use Avogadro's number and the molar mass of carbon. The periodic table tells us that the average molar mass of carbon is 12.011 g/mol. According to Avogadro's number, one mole of any substance contains exactly 6.022 × 1023 atoms.
Therefore, if one mole of carbon weighs 12.011 g, and contains 6.022 × 1023 atoms of carbon, then in 1.00 g of carbon, there would be a proportionally fewer number of atoms. The conversion is a straightforward one-step process:
1.00 g C × (6.022 × 1023 atoms C / 12.011 g C) = 5.02 × 1022 atoms C.
Thus, there are approximately 5.02 × 1022 atoms of carbon in 1.00 g of carbon.
The number of atoms of carbon in 1.00 g can be calculated using the molar mass of carbon and Avogadro's number. The molar mass of carbon is 12.011 g/mol and Avogadro's number is 6.022 × 1023 atoms/mol. To calculate the number of atoms, we can use the equation:
1.00 g C * (1 mol C / 12.011 g C) * (6.022 × 1023 atoms C / 1 mol C) = 5.02 × 1022 atoms C.