Final answer:
When 1.0000 g of Al reacts, it forms approximately 17.56 g of alum, based on the molar masses of Al (26.98 g/mol) and alum (474 g/mol). The provided answer choices do not match this calculation, suggesting a potential error in the problem or the answer choices.
Step-by-step explanation:
To calculate the mass of alum produced when 1.0000 g of Al reacts, we start by understanding the mole-to-mass relationship. The molar mass of alum is 474 grams. Next, we establish that the molar mass of aluminum (Al) is 26.98 grams per mole.
We use this information to determine how many moles of Al are present in 1 g:
- 1 mol Al / 26.98 g Al
- 1 g Al x (1 mol Al / 26.98 g Al) = 0.03705 mol Al
Assuming Al reacts in stoichiometric amounts to form alum, the same number of moles of Al will form moles of alum, because the ratio according to the balanced chemical equation is 1:1.
Now, we convert the moles of alum to grams using the molar mass of alum:
- 0.03705 mol Al x (474 g alum / 1 mol alum) = approximately 17.56 g of alum
None of the given answer choices match this calculation, which suggests there may be an error in the problem or the provided answer choices. However, if assuming that the mass of alum produced is directly proportional to 1.0000 g of Al, the closest approximate answer choice would be (a) Approximately 53.24 g.