So, a right workshift in equilibrium, while increasing concentration of our products, any of the products of both the products shifts our equilibrium to the left. So, increasing this guy will shift our equilibrium to the left, producing more of our reactants. So, why is that? Well, let's see once again, what happens when we increase the concentrations of this guy and this guy. Well, recall what the reaction quotient states. If you increase the concentration of our reactants, then our reaction quotient will become larger than our equilibrium constant K. And if Q is larger than K, that means we're going to observe a rightward shift in equilibrium in other words, the forward reaction will proceed this way at a higher rate than the reverse reaction.