[Intrud3r]

Hi, I'm currently revising for my final chem exams and i was skimming through some old papers. I came across a question with the following equation:

Cl2 + H2O <--> HOCl + H(+) + Cl(-)   

It asked me a quesiton along the following lines: If we were to acidify the system by the addition of nitric acid. What would happen to the rate of the forward reaction? By looking at it at first glance i said it was the forward reaction would decrease and backward would increase. But the answers say that it has no effect, or it will increase, which is right? Isn't the concentration of the H(+) ions being increased and thus the reverse reaction is favoured? Or does the increase in concentration of a single product/reactant have no effect on the rates of reaction??

Any insight into this problem would be much appreciated. Thanks in advance for the speedy reply.

Regards
Confused Student.

[Borek]

The question asks about RATE of forward reaction, you are discussing EQUILIBRIUM.

[Intrud3r]

Yes, but for the equilibrium to move, doesn't 1 reaction have to occur quicker than the other, so that the equilibrium changes. Otherwise won't it just be the same? Because if you increase the concentration of the Cl2, the forward reaction increases. So if you increase the concentration of the H(+) shouldn't the rate of the reverse reaction increase as well?

[Intrud3r]

Oh wait, i understand now. The reverse reaction rate increases, however the forward one stays the same, and increases slightly when more species have formed on the reactant side. All makes sense now. Thanks