Equilibrium

[Nicolas Williams]

Can someone explain what happens when Q>K and vice versa? As well as what this means for the equilibrium of the equation.

[Charlotte Norris 2K]

when Q>K, the reation is lying on the products side versus on the reactants side when Q<K and at equilibrium when Q=K

[005917072]

If Q>K, then there's more products at that point than there will be at equilibrium, so the reverse reaction will be favored and more reactants will be made. If Q<K, then there's more reactants at that point than there will be at equilibrium, so the forward reaction will be favored and more products will be made.

[Hansika_Sakshi_2k]

when Q>K the reaction will shift left creating more reactants. When Q<K the reaction will shift right creating more products and this is because Q to K ratio tells us if products or reactants increase which means the reaction needs to proceed with this new increase.