According to my textbook,

Increasing the concentration of the reactants increases the rate of forward reaction only to reestablish equilibrium (Le Chatelier's principle)

But doesn't that also increase the rate of the backwards reaction as products are produced?

  • 4
    $\begingroup$ It does, to an extent. As both rates become equal again, the new equilibrium is established. $\endgroup$ Feb 11 at 12:56
  • $\begingroup$ Yes, and both product and reactant concentrations are higher at the new equilibrium concentrations. That means that both the forward and reverse reaction rates are higher at the new equilibrium position but are still equal. $\endgroup$
    – user123462
    Feb 11 at 13:22
  • 4
    $\begingroup$ Please always include a proper citation when you quote a source. $\endgroup$ Feb 11 at 15:59
  • 1
    $\begingroup$ Yes, you are correct. The equilibrium constant is just that i.e. constant (at a given temperature), thus if $A=B$ then $K=[A]/[B]$ so if A increases so must B. $\endgroup$
    – porphyrin
    Feb 11 at 17:34
  • 1
    $\begingroup$ What textbook did you quote from? $\endgroup$
    – Buck Thorn
    Feb 15 at 6:08


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