Forward rate=Reverse rate


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Joe Zaarour 2L
Posts: 21
Joined: Fri Sep 25, 2015 3:00 am

Forward rate=Reverse rate

Postby Joe Zaarour 2L » Thu Feb 18, 2016 1:00 am

At equilibrium, why does the forward rate=the reverse rate. If K>1, shouldn't the forward rate be greater than the reverse rate because there are more products formed than reactants?

Matthew Gutierrez 2D
Posts: 19
Joined: Fri Sep 25, 2015 3:00 am

Re: Forward rate=Reverse rate

Postby Matthew Gutierrez 2D » Thu Feb 18, 2016 11:36 am

I am not sure if I'm understanding your question correctly.
At equilibrium, there is no net change in the concentrations of the reactants and products because the forward and reverse reaction rates are equal.
Equilibrium could also favor a larger concentration of reactants.
Please correct me if I am wrong!

JasmineAlberto4J
Posts: 73
Joined: Fri Sep 25, 2015 3:00 am

Re: Forward rate=Reverse rate

Postby JasmineAlberto4J » Thu Feb 18, 2016 11:46 am

K is based off of the concentrations of products and reactants. If a reaction is at equilibrium, the rate of that the forward reaction is occurring is equal to the rate that the reverse reaction is occurring. For a reaction to be at equilibrium, the concentrations of the products don't have to equal each other and this is why K isn't always 1. In sum, equilibrium is independent of the concentration, K is a ratio of the concentrations of the products to reactants.


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