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?

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  1. 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. 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.

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