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22 October, 11:00

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. If 10.6 grams of aluminum hydroxide is produced, how many grams of water were reacted?

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  1. 22 October, 11:23
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    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
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