Question

Most metals are very reactive, as are the elements in the halogen group. Aluminum, for instance, For example, reacts with elemental chlorine to form aluminum chloride. If you have a 13.5 g sample of Al, which choice below is true?

A. you will need 23.6 g Cl2 for complete reaction and will produce 66.7 g of AlCl3.
B. you will need 53.2 g Cl2 for complete reaction and will produce 66.7 g of AlCl3.
C. you will need 11.8 g Cl2 for complete reaction and will produce 49.0 g of AlCl3.
D. you will need 26.6 g Cl2 for complete reaction and will produce 49.0 g of AlCl3. Reset Selection

Answer 1

Answer: B. you will need 53.2 g Cl2 for complete reaction and will produce 66.7 g of AlCl3.

Step-by-step explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number
`6.023* 10^(23)` of particles.

To calculate the moles, we use the equation:

`\text{Number of moles of aluminium}=\frac{\text{Given mass}}{\text {Molar mass}}=(13.5g)/(27g/mol)=0.5moles`

The balanced reaction is:

`2Al+3Cl_2(g)\rightarrow 2AlCl_3`

2 moles of aluminium react with= 3 moles of chlorine

Thus 0.5 moles of aluminium react with=
`(3)/(2)* 0.5=0.75` moles of chlorine

Mass of chlorine=
`moles* {\text{Molar Mass}}=0.75* 71=53.2g`

2 moles of aluminium produce = 2 moles of aluminium chloride

Thus 0.5 moles of aluminium react with=
`(2)/(2)* 0.5=0.5` moles of aluminium chloride

Mass of aluminium chloride=
`moles* {\text{Molar Mass}}=0.5* 133.34=66.7g`

Thus 53.2 g of chlorine is used and 66.7 g of aluminium chloride is produced.