Exhibit 3-2 Aluminum sulfide, Al₂S₃ (molar mass = 150.16 g/mol) , reacts with water to form the aluminum hydroxide, Al(OH) ₃ (molar mass = 78.00 g/mol) , and hydrogen sulfide, H₂S, as shown below:
__ Al₂S₃ + __ H₂O→__ Al(OH) ₃ + __ H₂S (unbalanced reaction)
Refer to Exhibit 3-2. How many grams of aluminum hydroxide, Al(OH) ₃, is obtained from 10.5 g of aluminum sulfide, Al₂S₃?

Question

Quizplus · Accepted Answer

10.5 g Al2S3 x (1 mol Al2S3 / 150.16 g Al2S3) x (2 mol Al(OH)3 / 1 mol Al2S3) x (78.00 g Al(OH)3 / 1 mol Al(OH)3) = 10.9 g Al(OH)3

Exhibit 3-2 Aluminum Sulfide, Al2S3 (Molar Mass = 150

Exhibit 3-2 Aluminum Sulfide, Al₂S₃ (Molar Mass = 150