Final answer:
To determine the number of carbon atoms in 10.0 g of C2H6, calculate the number of moles from the mass and molar mass, and then multiply by Avogadro's number and the number of carbon atoms per molecule of ethane. This results in approximately 4.015 × 1023 carbon atoms.
Step-by-step explanation:
To find out how many carbon atoms are in 10.0g of C2H6, we first need to calculate the molar mass of ethane (C2H6). The molar mass is the sum of the masses of all the atoms in a molecule. Carbon has a molar mass of approximately 12 g/mol, and hydrogen has a molar mass of about 1 g/mol. Therefore, the molar mass of C2H6 is (2 × 12 g/mol) + (6 × 1 g/mol) = 30 g/mol.
Next, we calculate how many moles of C2H6 are in 10.0 g of the substance using the molar mass:
Number of moles of C2H6 = mass ÷ molar mass = 10.0 g ÷ 30 g/mol
This gives us approximately 0.333 moles of C2H6. Since each molecule of ethane contains 2 carbon atoms, we can find the total number of carbon atoms:
Total number of carbon atoms = number of moles of C2H6 × Avogadro's number × number of carbon atoms per molecule = 0.333 moles × 6.022 × 1023 atoms/mol × 2
Finally, this calculation will give us the total number of carbon atoms in 10.0 g of C2H6, which is approximately 4.015 × 1023 carbon atoms.