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I know that the activation energy of the forward reaction will decrease, but as for the reverse reaction I believe it is the same. I am not 100% sure about this, but I believe that the catalyst will not effect the reverse reaction activation energy unless it is built to do so (as most catalysts work to take specimens of higher Gibbs Free Energy to lower states, but there are some instances of the reverse.
Adding a catalyst will cause the activation energies of both the forward and reverse reactions to decrease, and it will cause the reaction rates of both the forward and reverse reactions to increase. There's a sapling problem that tests this exact question too! Hope that helps!
LeanneBagood_2F wrote:i understand why adding a catalyst will decrease the activation energy for the forward reaction, but im a bit confused as to why it's the same for the reverse. can someone explain this please?
A catalyst will reduce the activation energy for the entire reaction in general, both forward and reverse. If you look at a reaction profile for example, the catalyst will lower that hump representing the overall activation energy. If you were to imagine the reaction going in reverse, that activation energy will still be lower than the original activation energy. Hope that helps!
Catalysts lower the activation energy of a reverse reaction, as well as the forward reaction, because it orients the reactant molecules in a way where it can collide with enough energy to overcome the energy barrier.
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