Question at position 2 A sample of an oxide of vanadium is separated into its elements, resulting in 1.02 g V and 0.48 g O. Which of the following is the formula of the oxide?V2OV2O5V2O3VO2

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Question at position 2 A sample of an oxide of vanadium is separated into its elements, resulting in 1.02 g V and 0.48 g O. Which of the following is the formula of the oxide?V2OV2O5V2O3VO2

BlackTom AI · Accepted Answer

The task is to find the empirical formula of an oxide of vanadium from the masses of V and O obtained after separation.
First, determine the moles of each element from the given masses: vanadium mass = 1.02 g and vanadium atomic weight ≈ 50.94 g/mol, so n(V) = 1.02 / 50.94 ≈ 0.0200 mol. Oxygen mass = 0.48 g and oxygen atomic weight ≈ 16.00 g/mol, so n(O) = 0.48 / 16.00 = 0.0300 mol.
Next, compare the mole ratio by dividing both by the smaller number of moles: 0.0200 mol is the smaller, so n(V)/n(min) ≈ 0.0200 / 0.0200 = 1, and n(O)/n(min) ≈ 0.0300 / 0.0200 = 1.5. A 1:1.5 ratio translates to 2:3 when scaled to whole numbers (multiply both by 2).
Thus the empirical formula is V2O3.
Now evaluate the provided options one by one:
- Option A: V2O. This would correspond to a V:O ratio of 2:1, not matching the calculated 2:3, so it is incorrect.
- Option B: V2O5. This implies a V:O ratio of 2:5, far from 2:3; the oxygen content is too high relative to vanadium, so this is incorrect.
- Option C: V2O3. This matches the derived 2:3 ratio exactly, so this is the correct empirical formula.
- Option D: VO2. This corresponds to a 1:2 ratio, again not matching the calculated 2:3, so it is incorrect.
In summary, the mass data lead to a V:O mole ratio of approximately 1:1.5, which simplifies to 2:3, confirming V2O3 as the correct formula.

Question at position 2 A sample of an oxide of vanadium is separated into its elements, resulting in 1.02 g V and 0.48 g O. Which of the following is the formula of the oxide?V2OV2O5V2O3VO2

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