A vitamin A sample contains 2.0 x 1022 atoms of carbon. What is the mass of the vitamin A sample?[?] grams C20H30OReport your answer with the appropriate number of significant figures.

To solve this problem, we need to follow these steps:

1. Determine the number of carbon atoms in one molecule of Vitamin A. Vitamin A has a molecular formula of C20H30O, which means there are 20 carbon atoms in one molecule of Vitamin A.

2. Calculate the number of Vitamin A molecules in the sample. Since there are 2.0 x 10^22 carbon atoms and each Vitamin A molecule contains 20 carbon atoms, the number of Vitamin A molecules is (2.0 x 10^22) / 20 = 1.0 x 10^21 molecules.

3. Determine the molar mass of Vitamin A. The molar mass of carbon (C) is approximately 12.01 g/mol, hydrogen (H) is approximately 1.01 g/mol, and oxygen (O) is approximately 16.00 g/mol. So, the molar mass of Vitamin A is (2012.01 g/mol) + (301.01 g/mol) + (16.00 g/mol) = 286.5 g/mol.

4. Calculate the mass of the Vitamin A sample. Since there are 1.0 x 10^21 molecules of Vitamin A and 1 mole of any substance contains approximately 6.022 x 10^23 molecules (Avogadro's number), the number of moles of Vitamin A is (1.0 x 10^21) / (6.022 x 10^23) = 0.00166 moles. Therefore, the mass of the Vitamin A sample is (0.00166 moles) * (286.5 g/mol) = 0.476 g.

So, the mass of the Vitamin A sample is 0.476 grams.