Verified answer

To find the molecular formula of the oxide of silicon, we can use the concept of molar mass and stoichiometry.

1. First, calculate the mass of silicon used in the experiment:

  Mass of crucible + silicon - Mass of crucible = 15.28 g - 15.20 g = 0.08 g

2. Next, calculate the mass of oxygen that combined with silicon to form the oxide:

  Mass of crucible + oxide of silicon - Mass of crucible = 15.80 g - 15.20 g = 0.60 g

3. Now, we need to determine the number of moles of silicon and oxygen. To do this, we'll use their respective molar masses:

  - The molar mass of silicon (Si) is approximately 28.09 g/mol.

  - The molar mass of oxygen (O) is approximately 16.00 g/mol.

  Moles of silicon = (0.08 g) / (28.09 g/mol) ≈ 0.00285 moles

  Moles of oxygen = (0.60 g) / (16.00 g/mol) ≈ 0.0375 moles

4. Now, we need to determine the mole ratio of silicon to oxygen. Divide the moles of silicon by the smaller number of moles, which is approximately 0.00285:

  Mole ratio of Si to O ≈ (0.00285 moles Si) / (0.00285 moles Si) = 1

  Mole ratio of O to Si ≈ (0.0375 moles O) / (0.00285 moles Si) ≈ 13.16

5. The mole ratio of Si to O is approximately 1, and the mole ratio of O to Si is approximately 13.16.

6. To get whole numbers for the mole ratio, we can round the ratio to the nearest whole number. In this case, the ratio of O to Si is approximately 13.16, which can be rounded to 13.

7. The molecular formula of the oxide of silicon is SiO13.

So, the molecular formula of the oxide of silicon is SiO13.

Explanation:

First, we need to find the mass of Tin (Sn) and Oxygen (O) in the Tin Oxide sample. Mass of Tin (Sn) = (Mass of crucible, cover, and Tin sample) - (Mass of crucible and cover) Mass of Tin (Sn) = 21.08 g - 18.98 g = 2.10 g Mass of Oxygen (O) = (Mass of crucible, cover, and Tin Oxide) - (Mass of crucible, cover, and Tin sample) Mass of Oxygen (O) = 21.93 g - 21.08 g = 0.85 g