Final answer:
The calculation of the maximum number of moles and grams formed in a reaction requires the molar mass of the substances and the quantities of the reactants. Without specifying the amount of aluminum sulfide and water, it's not possible to provide an exact answer.
Step-by-step explanation:
To calculate the maximum number of moles and grams of product formed when aluminum sulfide reacts with water, a stoichiometric calculation is needed. Assuming the reaction is:
Al2S3 + 6H2O → 2Al(OH)3 + 3H2S,
which is a similar type of reaction to those shown in the provided information. We'll need the molar mass of the substances involved and the mass of water in grams to determine the moles of water. One critical aspect of the stoichiometry is identifying the limiting reactant - the reactant that will be completely consumed first and therefore limits the amount of product that can be formed.
In the examples provided, the corresponding quantities of reactants were converted into moles, and the stoichiometry of the reaction was used to determine the amount of the product. Here, the question seems to miss specific amounts for aluminum sulfide and water; therefore, without these values, we cannot provide the exact number of moles or grams. To answer the question accurately, the amount of aluminum sulfide in moles and the mass of water in grams need to be specified.