- #1
chemkid1234
- 7
- 0
Hey guys,
I have a question regarding the process by which a reaction returns to equilibrium.
If a reaction's reaction quotient is greater than its equilibrium constant, it will shift towards the reactants side of the equation to return to equilibrium. How exactly does this happen? Does the forward reaction stop, or does the rate of the reverse reaction increase so reactants are being produced quicker than products? Is there ever a point where products or reactants are not being produced at all?
I have a question regarding the process by which a reaction returns to equilibrium.
If a reaction's reaction quotient is greater than its equilibrium constant, it will shift towards the reactants side of the equation to return to equilibrium. How exactly does this happen? Does the forward reaction stop, or does the rate of the reverse reaction increase so reactants are being produced quicker than products? Is there ever a point where products or reactants are not being produced at all?