Final answer:
After calculating the moles of tin and oxygen, the empirical formula of the tin oxide is determined to be SnO₂, which is named stannic oxide. Option B, SnO₂; stannic oxide, is the correct answer.
Step-by-step explanation:
To calculate the empirical formula of the tin oxide produced when a 0.430 g sample of tin metal reacts with oxygen to achieve a final mass of 0.546 g, we first need to determine the mass of oxygen that reacted with the tin. This is found by subtracting the mass of the tin from the final mass of the tin oxide: 0.546 g - 0.430 g = 0.116 g of oxygen.
Next, we convert the masses of tin and oxygen to moles using their respective atomic masses (Sn: 118.71 g/mol, O: 16.00 g/mol):
- moles of Sn = 0.430 g / 118.71 g/mol = 0.00362 moles of Sn
- moles of O = 0.116 g / 16.00 g/mol = 0.00725 moles of O
Now, we need to find the simplest whole number ratio of moles of Sn to moles of O by dividing by the smallest number of moles:
- ratio of Sn to O = 0.00362 moles Sn / 0.00362 = 1
- ratio of O to Sn = 0.00725 moles O / 0.00362 ≈ 2
Therefore, the empirical formula of the tin oxide is SnO₂.
The correct name for SnO₂ is stannic oxide as tin has a valence of +4 in this compound, thus option B is the correct answer: