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Fynjy0 [20]
2 years ago
8

Use the reaction given below to solve the problem that follows: Calculate the mass in grams of aluminum oxide produced by the re

action of 15.0 g of aluminum metal.
[ ]grams Al2O3

4 Al + 3 O2 --> 2 Al2O3

**Your answer should be written as XX.X
Chemistry
1 answer:
bearhunter [10]2 years ago
7 0

Answer:  28.4 g of aluminum oxide is produced by the reaction of 15.0 g of aluminum metal

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}   

\text{Moles of} Al=\frac{15.0g}{27g/mol}=0.556moles

The balanced chemical equuation is:

4Al+3O_2\rightarrow 2Al_2O_3  

According to stoichiometry :

4 moles of Al produce == 2 moles of Al_2O_3

Thus 0.556 moles of Al will produce=\frac{2}{4}\times 0.556=0.278moles  of Al_2O_3

Mass of Al_2O_3=moles\times {\text {Molar mass}}=0.278moles\times 102g/mol=28.4g

Thus 28.4 g of aluminum oxide is produced by the reaction of 15.0 g of aluminum metal.

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<h3>What are IUPAC names?</h3>

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Explanation:

Just saw your request regarding answering this so here it is:

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