# Chemistry: Equilibrium

Hello there. I'm having trouble understanding equilibrium. Especially understanding if the reactions go foward or reverse when there is a change in tempertature, concentration, pressure/volume etc. For example:

In a solution of copper (II) chloride, the following equilibrium exists.

$$CuCl_4^{2-}_{(aq)} + 4H_2O_{(l)} \rightleftharpoons Cu(H_2O)_4^{2+}_{(aq)} + 4Cl^{-}_{(aq)}$$

For the following stresses put on the equilirbrium, predict the shift in the equilibrium.

1) Would this be a reverse reaction since the acid dissociates into $$HCl_{(aq)} \rightarrow H^{+}_{(aq)} + Cl^{-}_{(aq)}$$? So the concentration of Cl will be increased and it will shift to the left?

2)I think it's a reverse reaction but I'm not sure. Why would it be a reverse reaction (or foward if I'm wrong)? Thanks for the help.

erik05 said:
Hello there. I'm having trouble understanding equilibrium. Especially understanding if the reactions go foward or reverse when there is a change in tempertature, concentration, pressure/volume etc. For example:

In a solution of copper (II) chloride, the following equilibrium exists.

$$CuCl_4^{2-}_{(aq)} + 4H_2O_{(l)} \rightleftharpoons Cu(H_2O)_4^{2+}_{(aq)} + 4Cl^{-}_{(aq)}$$

For the following stresses put on the equilirbrium, predict the shift in the equilibrium.

1) Would this be a reverse reaction since the acid dissociates into $$HCl_{(aq)} \rightarrow H^{+}_{(aq)} + Cl^{-}_{(aq)}$$? So the concentration of Cl will be increased and it will shift to the left?