Final answer:
The further a reaction is from equilibrium, the greater its capacity to do work. Equilibrium is the state where reactants and products are formed at equal rates. Activation energy and temperature significantly influence reaction rates, while catalysts can increase the rate by lowering the activation energy.
Step-by-step explanation:
The further a reaction is kept away from equilibrium, the more capacity it has to do work. In chemistry, equilibrium is the point at which the reactants and products of a chemical reaction are formed at the same rate, so no net change occurs in the concentrations of the reactants and products. Keeping a reaction away from equilibrium means that there is a higher potential to do work, as the reaction is either absorbing energy or releasing energy until it reaches equilibrium.
The concept of activation energy is also crucial, as this is the minimum amount of energy required to start a chemical reaction. At higher temperatures, more molecules have the kinetic energy needed to overcome the activation energy barrier, leading to a faster reaction rate. Using a catalyst can lower the activation energy required, thereby increasing the rate at which equilibrium is achieved without affecting the position of the equilibrium.