# Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. write a balanced equation for this reaction.

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. write a balanced equation for this reaction. how many grams of aluminum hydroxide can be obtained from 5.50g of aluminum sulfide?

## This Post Has 2 Comments

1. mduncan840 says:

There reacts 7.35 grams of H2O

Explanation:

Step 1: Data given

Mass of aluminium hydroxide = 10.6 grams

Step 2: The balanced equation

Al2S3(s) + 6H2O(l) → 2Al(OH)3(s) + 3H2S(g)

Step 3: Calculate number of moles Al(OH)3

Moles Al(OH)3 = mass Al(OH)3 / molar mass Al(OH)3

Moles Al(OH)3 = 10.6 grams / 78.00 g/mol

Moles Al(OH)3 = 0.136 moles

Step 4: Calculate moles of H2O

For 1 mol of Al2S3 we need 6 moles of H2O to produce 2 moles of Al(OH)3 and 3 moles of H2S

For 0.136 moles of Al(OH)3 we need 3*0.136 = 0.408 moles of H2O

Step 5: Calculate mass of H2O

Mass H2O = moles H2O * molar mass of H2O

Mass H2O = 0.408 * 18.02 = 7.35 grams

There reacts 7.35 grams of H2O

2. fatherbamboo says:

This type of reaction is a metathesis. It involves double replacement of two reactants to yield two products, one of which is an insoluble product called precipitate. In this case, the complete balanced reaction would be

Al2S3(s) + 6 H2O(l) ⇒ 2 Al(OH)3 (aq) + 3 H2S(s)

Aluminum Sulfide (Al2S3) in room conditions is a solid. When it is dissolved in water, it creates an aqueous solution of Aluminum Hydroxide (Al(OH)3). The insoluble precipitate produced is a solid form of Hydrogen Sulfide (H2S). To know the phase of the reactants, you can refer to the Material Safety Datasheets to know the property characteristics of various elements and compounds.