To determine the number of hydrogen atoms in 1.7 g of H2O2 (hydrogen peroxide), we need to consider the molar mass of H2O2 and the Avogadro's number.
The molar mass of H2O2 can be calculated by adding the atomic masses of its constituent elements: 2 hydrogen atoms (H) and 2 oxygen atoms (O). The atomic masses (also known as atomic weights) can be found in the periodic table.
The atomic mass of hydrogen (H) is approximately 1.00784 g/mol, and the molecular mass of oxygen (O) is approximately 15.999 g/mol.
Molar mass of H2O2: (2 × Atomic mass of hydrogen) + (2 × Atomic mass of oxygen) = (2 × 1.00784 g/mol) + (2 × 15.999 g/mol) ≈ 2.01568 g/mol + 31.998 g/mol ≈ 34.01368 g/mol
Now, we can calculate the number of moles of H2O2 present in 1.7 g by using the formula:
Number of moles = Mass / Molar mass
Number of moles of H2O2 = 1.7 g / 34.01368 g/mol ≈ 0.05 mol
Since each molecule of H2O2 contains two hydrogen atoms, the number of hydrogen atoms can be calculated by multiplying the number of moles by Avogadro's number (6.02214076 × 10^23 atoms/mol):
Number of hydrogen atoms = Number of moles × Avogadro's number ≈ 0.05 mol × (6.02214076 × 10^23 atoms/mol) ≈ 3.01107038 × 10^22 hydrogen atoms
Therefore, there are approximately 3.01107038 × 10^22 hydrogen atoms in 1.7 g of H2O2.