Question

Use the reaction given below to solve the problem that follows: Calculate the mass in grams of aluminum oxide produced by the reaction of 15.0 g of aluminum metal.

[ ]grams Al2O3

4 Al + 3 O2 --> 2 Al2O3

**Your answer should be written as XX.X

Answer 1

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

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} Al=(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=
`(2)/(4)* 0.556=0.278moles` of
`Al_2O_3`

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

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