The term -\fracE_aRT is commonly found in the context of chemical kinetics and thermodynamics. Here, E_a represents the activation energy, which is the minimum energy required for a chemical reaction to occur. The negative sign indicates that as the activation energy increases, the rate of the reaction decreases, reflecting the energy barrier that must be overcome. In this equation, R is the universal gas constant, and T is the absolute temperature in Kelvin. This relationship helps to explain how temperature influences reaction rates. As temperature increases, the value of -\fracE_aRT becomes less negative, leading to a higher reaction rate due to more molecules having sufficient energy to overcome the activation barrier.