When a reversible reaction takes place in a closed container, the mixture eventually reaches equilibrium. The rate of attainment of equilibrium means how quickly this happens. Anything that makes the reactions go faster means equilibrium is reached sooner.
Temperature: at a higher temperature the particles move faster, so they collide more often and with more energy. More of the collisions succeed, so equilibrium is reached faster. Lowering the temperature has the opposite effect, and equilibrium is reached more slowly.
Pressure and concentration: for reactions involving gases, a higher pressure squeezes the particles closer together. A higher concentration of a dissolved reactant also puts more particles in the same volume. In both cases the particles collide more often, so equilibrium is reached faster.
Catalyst: a catalyst lowers the energy needed for the reaction. It speeds up the forward reaction and the backward reaction by the same amount, so equilibrium is reached faster. It does not change the amount of product in the equilibrium mixture. This lesson is about how fast equilibrium is reached, not about how much product there is.