Equilibrium Reaction HELP!?!?!

I really don't understand this question

Here's the equation:
2CrO4(2-)(aq) + 2H(1+)(aq) <> Cr2O(2-)7(aq) + H2O(l)

where the numbers in the brackets are the charge and (aq) means aqueous solution and (l) is liquid

1) What effect will increasing the dichromate ion have on the equilibrium?
2) What effect will adding HCl have on the equilibrium?

Number 2 has something to do with the HCl splitting into H+ and Cl- but I don't quite get it.

And please explain why I don't understand how ions affect the equilibrium.

I'll definitely be giving away the 10 points to whoever helps me understand or puts the most effort in their answer, so please answer :)

1.) If we increase Dichromate ion [Cr2O(2-)7], that is, if we increase one of the product, then using Le Chatlier's principle, equilibrium will shift towards left side.

2.) HCl is a strong acid, it will dissociate into H+ and Cl-, thus increasing H+ concentration on left side. This means reactant will increase, and hence it will try to make more product.

The dichromate ion is CrO4(^2-) and appears on the left side of the equation. Increasing the dichromate concentration will then shift the equilibrium to the right (from LeChatelier's principle, the equilibrium will shift so as to oppose the change).

You are right, HCl ionizes completely into H+ and Cl- ions, so adding HCl is adding H+ ions. H+ appears on the left side of the equation, so adding H+ will shift the equilibrium to the right as described above.

In both cases the result will be that more reaction products will be formed.

You need to use Le Chateliers principle, which states that if you have a system in equilibrium and you change the conditions the equilibrium will shift in such a way as to try to undo the change you made. Thus if you add dichromate ion the equilibrium will shift to the right, which removes dichromate. Similarly for H+.HCl reacts with water to form H3O+ and Cl- (H+ is shorthand for H3O+) so if you add HCl to the solution you are adding H+ and Cl-