Question

so I don't expect you to answer all of these I just don't understand how they work so if someone could just explain one or two so I can do the rest that would be helpful! Thanks!

Use the activity series to predict whether the following reaction will occur. Enter the products in the balanced reaction (as chemical symbols). Where no reaction will occur enter "no reaction" as the product.:

a) Zn + H2SO4

b) 2 AlI3 + 3 Cl2

b) Mg + 2 AgNO3

c) 2 Al + 3 CoSO4

Answer 1

All of these are single replacement reactions IF they occur. The secret to knowing i they occur is to use the activity series as the prelude in the question suggests. If you don't have a copy of the activity series you can see one at this link.

http://www.files.chem.vt.edu/RVGS/ACT/notes/activity_series.html

If the free metal is ABOVE the metal ion in the compound, the reaction will occur. If the free metal is not above the metal ion in the compound there will not be a reaction. It's that simple.;
For example, Zn is ABOVE H^+ (in H2SO4--I know H isn't a metal but it's the positive ion being replaced); therefore, the reaction will proceed as follows:
Zn + H2SO4 ==> ZnSO4 + H2

Mg is ABOVE Ag in the activity series; a reaction will occur.
Mg + 2AgNO3 ==> Mg(NO3)2 + 2Ag

A couple of other examples.
Cu + AgNO3 ==> ?
Cu is ABOVE Ag; therefore, the reaction is Cu + 2AgNO3 ==> Cu(NO3)2 + 2Ag

and
Ag + Cu(NO3)2 ==> No Reaction BECAUSE Ag is BELOW Cu in the activity series.