Final answer:
To find the number of carbon atoms in 1.0g of Na2CO3, calculate the moles of Na2CO3 using its molar mass (105.99 g/mol), and then multiply by Avogadro's number (6.022 × 10^23 atoms/mole) to obtain approximately 5.68 × 10^21 atoms of carbon.
Step-by-step explanation:
To determine how many atoms of carbon are present in 1.0g of Na2CO3, we first need to calculate the moles of Na2CO3 in 1.0g. The molar mass of Na2CO3 is the sum of the molar masses of its constituent elements: (2 × 22.99) + 12.01 + (3 × 16.00) = 105.99 g/mol. Thus, 1.0g of Na2CO3 is equivalent to 1.0g / 105.99g/mol = 9.44 × 10-3 moles of Na2CO3.
Since each mole of Na2CO3 contains one mole of carbon atoms, and Avogadro's number tells us that there are 6.022 × 1023 atoms in a mole, we can multiply the moles of Na2CO3 by Avogadro's number to find the number of carbon atoms.
Therefore, the number of carbon atoms in 1.0g of Na2CO3 is:
9.44 × 10-3 moles × 6.022 × 1023 atoms/mole = 5.68 × 1021 atoms of carbon.