Activatied complex: molecules for a reaction “prepared” f = The fraction of molecules that have an energy equal or greater to Ea Arrhenuis Equation Calculating the Activation Energy for a Reaction Rearrange the Arrhenius Equation Utilize reaction data Example: Using Arrhenius Calculate the activation energy (Ea) for the reaction N2O5(g) 2NO2(g) + ½ O2(g) → from the observed rate constants at the following two temperatures: (a) at 25oC, k = 3.46x10-5s-1 and (b) at 55oC, k = 1.5x10-3s-1. Assignment #3: The Arrhenius Equation the hypothetical reaction A + B + D, the activation energy is 32 kJ/mol. For the reverse C reaction(C+DA+B),the activation energy is 58kJ/mol. Is the reaction A+BC+D exothermic or endothermic? Justify your answer. the activation energy (Ea) for the reaction N2O5(g) + 1⁄2 O2(g), from the observed rate 2NO2(g) constants at the following two temperatures: (a) at 25oC, k = 3.46x10-5 s-1 (b) at 55oC, k = 1.5x10-3 s-1
Activatied complex: “prepared” molecules for a reaction f = The fraction of molecules that have an energy equal or greater to Ea Arrhenuis Equation Calculating the Activation Energy for a Reaction Rearrange the Arrhenius Equation Utilize reaction data Example: Using Arrhenius Calculate the activation energy (Ea) for the reaction N2O5(g) → 2NO2(g) + ½ O2(g) from the observed rate constants at the following two temperatures: (a) at 25oC, k = 3.46x10-5s-1 and (b) at 55oC, k = 1.5x10-3s-1. Assignment #3: The Arrhenius Equation the hypothetical reaction A + B C + D, the activation energy is 32 kJ/mol. For the reverse reaction(C+DA+B),the activation energy is 58kJ/mol. Is the reaction A+BC+D exothermic or endothermic? Justify your answer. the activation energy (Ea) for the reaction N2O5(g) 2NO2(g) + 1⁄2 O2(g), from the observed rate constants at the following two temperatures: (a) at 25oC, k = 3.46x10-5 s-1 (b) at 55oC, k = 1.5x10-3 s-1