- #1
erik05
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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.
[tex] CuCl_4^{2-}_{(aq)} + 4H_2O_{(l)} \rightleftharpoons Cu(H_2O)_4^{2+}_{(aq)} + 4Cl^{-}_{(aq)} [/tex]
For the following stresses put on the equilirbrium, predict the shift in the equilibrium.
1) Hydrochloric acid is added
2) Silver nitrate is added.
1) Would this be a reverse reaction since the acid dissociates into [tex] HCl_{(aq)} \rightarrow H^{+}_{(aq)} + Cl^{-}_{(aq)} [/tex]? 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.
In a solution of copper (II) chloride, the following equilibrium exists.
[tex] CuCl_4^{2-}_{(aq)} + 4H_2O_{(l)} \rightleftharpoons Cu(H_2O)_4^{2+}_{(aq)} + 4Cl^{-}_{(aq)} [/tex]
For the following stresses put on the equilirbrium, predict the shift in the equilibrium.
1) Hydrochloric acid is added
2) Silver nitrate is added.
1) Would this be a reverse reaction since the acid dissociates into [tex] HCl_{(aq)} \rightarrow H^{+}_{(aq)} + Cl^{-}_{(aq)} [/tex]? 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.