Aluminum reacts with chlorine gas according to the following equation:

2 Al(s) + 3 Cl2(g) → 2 AlCl3(s)

How many moles of Cl2 are required to react with each mole of aluminum?

a. 1
b. 0.5
c. 1.5
d. 2.5
e. 2

For 1 moles Aluminium we need 3.0 / 2 = 1.5 moles Chlorine gas (Cl2)

Option C is correct

Explanation:

Step 1: data given

Aluminium = Al(s)

Chlorine gas = Cl2(g)

Step 2: The balanced equation

2 Al(s) + 3 Cl2(g) → 2 AlCl3(s)

Step 3: Calculate moles Cl2

For 2 moles Aluminium we need 3 moles chlorine gas to react, to product 2 moles AlCl3

For 1 moles Aluminium we need 3.0 / 2 = 1.5 moles Chlorine gas (Cl2)

Option C is correct

CuSO4 + Fe -> FeSO4 + Cu

Explanation:

This reaction is a classic example of a redox reaction. I won't go in too deep, but the basic thing is that electrons from the Fe atom go to the Cu2+ ion. Therefore, Fe becomes an ion, and Cu - an electroneutral atom:

Fe + Cu2+ -> Fe2+ + Cu.

Silver is not a very reactive metal and it does not give up its electrons to Cu.