Question

Aluminum chloride, AICh is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the following equation. 2 Aln + 3 Cla) → 2 AlCl3() a) If 13,49 g of Al and 35.45 g of Cl2 are allowed to react, how much AlCl is produced? b) How many grams of the excess reactant is left?!

Answer 1

a) 44.442 grams of aluminium chloride is produced.

b) 8.996 grams of the excess reactant that id aluminum is left unreacted.

Step-by-step explanation:

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

Moles of aluminum =
`(13.49 g)/(27 g/mol)=0.4996 mol`

Moles of chlorine gas =
`(35.45)/(35.5 g/mol)=0.4993 mol`

According to reaction, 1 mol aluminum reacts with 3 moles of chlorine gas.

Then 0.4996 moles of aluminum will react with:

`(3)/(1)* 0.4996 mol=1.4988 mol` of chlorine gas

Then 0.4993 moles of chlorine gas will react with:

`(1)/(3)* 0.4993 mol=0.1664 mol` of aluminum

As we can see that moles of an aluminium are in excess. Hence, aluminium is an excess reagent.

So moles of aluminum chloride will depend upon moles of chlorine gas.

According to reaction 3 moles of chlorine gas give 2 moles of aluminium chloride.

Then 0.4993 mole of chlorine gas will give:

`(2)/(3)* 0.4993 mol=0.3329 mol` of aluminium chloride .

Mass of 0.3329 moles of aluminium chloride :

=0.3329 mol × 133.5 g/mol= 44.442 g

44.442 grams of aluminium chloride is produced.

Moles of aluminium left unreacted = 0.4996 mol - 0.1664 mol = 0.3332 mol

Mass of 0.3332 moles of aluminum :

0.3332 mol × 27 g/mol = 8.996 g[/tex]

8.996 grams of the excess reactant that id aluminum is left unreacted.