OpenStudy (anonymous):
Hello. If you watch this video http://www.youtube.com/watch?v=qy3ua2SWyko&feature=autoplay&list=PLA11A67B3AF749AA1&playnext=1 the guy narrating explains how the activation energy is certain for a reaction to occur and the activation energy for a backward reaction is even higher. What I don't get that if this is always true, then how in an endothermic reaction, for which reverse reaction is exothermic so releasing energy in the form of bonds breaking in products, how could it be harder for the reaction to occur in reverse if theoretically particles would have to take less energy into themselves
OpenStudy (anonymous):
what the man was trying to say is that that particular diagram represents exothermic process and as you know exothermic process releases energy, so for reverse reaction to occur you need to add that energy (heat) and activation energy. i think maybe this diagram will clear some things up: http://www.saskschools.ca/curr_content/chem30_05/graphics/2_graphics/exo.gif
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