What mass of aluminium hydroxide is needed to decompose in order to produce 65.0 l of water at stp in stoichiometry?

                               2 Al(OH)₃    →    Al₂O₃  +  3 H₂O

The mass of aluminium hydroxide needed is 150.774 grams.

Explanation:

The chemical equation for the decomposition of aluminium hydroxide follows:

At STP:

22.4 L of volume is occupied by 1 mole of a gas.

So, 65 L of volume will be occupied by =

By Stoichiometry of the reaction:

3 moles of water is produced by 2 moles of aluminium hydroxide

So, 2.9 moles of water is produced by =

To calculate the mass of aluminium hydroxide, we use the equation:

Number of moles of aluminium hydroxide = 1.933 moles

Molar mass of aluminium hydroxide = 78 g/mol

Putting values in above equation, we get:

Hence, the mass of aluminium hydroxide needed is 150.774 grams.

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .

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