Reverse Reaction

[505997354]

In my notes, it states if products is being favored (Q>K), then reverse reaction is favored. Shouldn't be the opposite, if all the electrons are going to reactants now?

[Chris_1234]

The statement in your notes is correct. When the reaction quotient (Q) is greater than the equilibrium constant (K), it means that the concentration of products is higher than what the equilibrium state dictates. According to Le Chatelier's Principle, the system will shift to counteract the change. So, the reverse reaction will be favored to consume the excess products, reducing their concentration and restoring equilibrium. This shift ultimately reduces Q and brings it closer to K. Therefore, the statement aligns with the principle of equilibrium and the behavior of chemical systems.

[Valeria Perez 3J]

If products are being favored and Q>K, the reverse reaction proceeds in order to reach equilibrium again by raising the concentration of the reactants. A right shift in concentration causes the reaction to level itself out by going in the opposite direction. Hope that helps!

[Charlotte Norris 2K]

Since Q is a snapshot of where the reaction is currently, then being greater than the equilibrium constant means it is on the product side and in order to get back to equilibrium, the reverse reaction needs to proceed.