Calculate the number of \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{O}\) atoms in \(1.50 \mathrm{~g}\) of glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right),\) a sugar.

First, we need to calculate the molar mass of glucose (\(C_6H_{12}O_6\)) by adding up the molar masses of all its constituent atoms. The molar mass of Carbon (C) is 12.01 g/mol, Hydrogen (H) is 1.01 g/mol, and Oxygen (O) is 16.00 g/mol. Hence, the molar mass of glucose is \(6 \times 12.01 g/mol + 12 \times 1.01 g/mol + 6 \times 16.00 g/mol = 180.18 g/mol.\)

Next, we'll calculate the number of moles of glucose in the 1.50 g sample. We use the formula: Moles = mass / molar mass. Plugging in the given mass and the calculated molar mass, we get \(n = 1.50 g / 180.18 g/mol = 0.00832 mol\) (rounded to five decimal places).

Finally, we'll calculate the number of each type of atom in the sample. Since there are 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms in one molecule of glucose, we multiply the number of moles of glucose by Avogadro's number (approximately \(6.022 \times 10^{23} / mol\)) to get the number of glucose molecules, then multiply by the number of each type of atom. So, the number of carbon atoms = \(0.00832 mol \times 6.022 \times 10^{23} molecules/mol \times 6 = 2.99 \times 10^{23}\), the number of hydrogen atoms = \(0.00832 mol \times 6.022 \times 10^{23} molecules/mol \times 12 = 5.99 \times 10^{23}\), the number of oxygen atoms = \(0.00832 mol \times 6.022 \times 10^{23} molecules/mol \times 6 = 2.99 \times 10^{23}\).

After calculating, we can confirm that the numbers of carbon and oxygen atoms are the same, and the number of hydrogen atoms is twice the number of carbon or oxygen atoms, which matches the molecular formula of glucose (\(C_6H_{12}O_6\))