Forward rate=Reverse rate

[Joe Zaarour 2L]

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]

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]

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.