A key reaction in the upper atmosphere is O31g2 + O1g2 ¡ 2 O21g2 For this process, the energy of activation for the forward reaction, Ea1fwd2, is 19 kJ/mol, and the enthalpy change for the reaction, ΔHrxn, is -392 kJ>mol. What is the energy of activation for the reverse reaction, Ea1reverse2? (LO 14.10) (a) 411 kJ/mol (b) 392 kJ/mol (c) 373 kJ/mol (d) 196 kJ/mol

Video transcript

Hello everyone today we have the following problem. The following reaction is known to be an exit thermic process. Assume that the energy of activation for the forward and backward reactions are 15 kg per moles 330 kg per mole respectively, calculate the entropy change for the reaction overall. So before we do that, let's just note that for an exhaust thermic reaction it means there's going to be a release of heat, Excel means outside and thermic means related to heat. And so the eggs are thermic reaction or for an exit thermic reaction. The activation energy and the reverse direction is essentially the sum of the magnitudes of the activation energy and the forward position and the entropy change or the change in entropy for the reaction. So if we were to rearrange this, we could say that the change in entropy for the reaction is equal to the activation energy for the reverse reaction minus the activation energy for the forward reaction. However, this must be negative or entropy change has to be negative because there is a release of energy. And so if we were to plug in our values we have the activation energy of the reverse being 330. Kill it, jules per mole - The activation energy of the forward reaction which is 15 kg per mole. This gives us a value of 315 killed jules per mole. However, we have to determine that it is going to be negative because it is an exo thermic reaction. And so our final answer is going to be -315 kg per mole. And with that we've answered the question overall, I hope that this helped, and until next time.