Q and Spontaneity

[makenzie2K]

I'm having trouble grasping the concept of the change in Q with respect to the spontaneous reaction. I understand the relationship between Q and K but I don't see how this applies to "spontaneity" in forming products. Thanks!

[Iris Bai 2K]

If Q is less than K, that means there is a higher concentration of reactants than products compared to the respective concentrations at equilibrium. Since all systems want to be at equilibrium, this scenario would favor the forward reaction in order to decrease the reactant concentration, making the forward reaction spontaneous. This also applies vice versa.