How many grams of aluminium hydroxide can be contained from 5.50 grams of aluminium sulfide?

To determine how many grams of aluminum hydroxide can be produced from 5.50 grams of aluminum sulfide (Al₂S₃), we first need to know the balanced chemical reaction involved. The reaction between aluminum sulfide and water produces aluminum hydroxide and hydrogen sulfide. The molar mass of Al₂S₃ is approximately 150.17 g/mol, and that of aluminum hydroxide (Al(OH)₃) is about 78.00 g/mol. Using stoichiometry, 1 mole of Al₂S₃ produces 2 moles of Al(OH)₃; thus, from 5.50 g of Al₂S₃, we can calculate that it can yield approximately 7.30 grams of aluminum hydroxide.