Which of the following has the lowest mass?

Question

BlackTom AI · Accepted Answer

Question: Which of the following has the lowest mass?

First, note that the provided data includes only one explicit option in the answer field: 'b. 0.5 mol of AlF3'. There are no other answer options listed, so a complete comparison across all choices cannot be performed from the given information.

To compare masses across different options, you would generally convert each option to a mass in grams using the formula:
mass = number of moles × molar mass.

For the option given (0.5 mol of AlF3):
- Determine the molar mass of AlF3. Aluminum (Al) has an approximate atomic mass of 26.98 g/mol, and fluorine (F) has an atomic mass of about 19.00 g/mol. AlF3 consists of 1 Al atom and 3 F atoms, so:
  M(AlF3) ≈ 26.98 + 3×19.00 = 26.98 + 57.00 ≈ 83.98 g/mol.
- Mass of 0.5 mol of AlF3 ≈ 0.5 × 83.98 ≈ 41.99 g (roughly 42 g).

With only this option available, you can say that this option corresponds to a mass of about 42 g. However, to determine whether this is the lowest mass, you would need the masses of all other options for direct comparison.

If you later obtain the missing options, apply the same method to each:
- Find the molar mass of the species in each option.
- Multiply by the number of moles given in that option to get the mass in grams.
- Compare the resulting masses; the smallest value is the lowest mass among the options.

Common pitfalls to avoid: assuming that a smaller number of moles always means a smaller mass without considering the molar mass; some compounds have very high molar masses per mole (e.g., heavy metal-containing species), which can offset fewer moles.

Summary: From the available data, the mass corresponding to 0.5 mol of AlF3 is about 42 g. To determine definitively which option has the lowest mass, you need the rest of the answer choices to compare directly.

Which of the following has the lowest mass?

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