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nata0808 [166]
3 years ago
8

what mass of aluminium hydroxide is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry?

Chemistry
2 answers:
pishuonlain [190]3 years ago
6 0
Aluminium Hydroxide on decomposition produces Al₂O₃ and Water vapors. 

<span>                               2 Al(OH)</span>₃    →    Al₂O₃  +  3 H₂O


According to equation at STP,

       67.2 L (3 moles) of H₂O is produced by  =  78 g of Al(OH)₃
So,
                65.0 L of H₂O will be produced by  =  X g of Al(OH)₃

Solving for X,
                                 X  =  (65.0 L × 78 g) ÷ 67.2 L

                                 X  =  75.44 g of Al(OH)₂
Result:
           75.44 g of Al(OH)₂ is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry
tatyana61 [14]3 years ago
5 0

<u>Answer:</u> The mass of aluminium hydroxide needed is 150.774 grams.

<u>Explanation:</u>

The chemical equation for the decomposition of aluminium hydroxide follows:

2Al(OH)_3\rightarrow Al_2O_3+3H_2O

At STP:

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

So, 65 L of volume will be occupied by = \frac{1}{22.4L}\times 65L=2.9mol

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 = \frac{2}{3}\times 2.9=1.933mol

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

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Number of moles of aluminium hydroxide = 1.933 moles

Molar mass of aluminium hydroxide = 78 g/mol

Putting values in above equation, we get:

1.933mol=\frac{\text{Mass of aluminium hydroxide}}{78g/mol}\\\\\text{Mass of aluminium hydroxide}=150.774 grams

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

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