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If yes, by increasing the temperature, do I increase the successful collisions right?
@Photon336 if you have time. Help me. Thank you.
@korosh23 yeah sure no problem.
So that means I am correct?
Well, yes you see like that's what happens in any chemical reaction you have successful collisions between particles
what they mean by successful is that the particles collide with the sufficient orientation and energy
let's see why though |dw:1442770275751:dw|
Right Ea, the minimum energy for successful collision to result.
So on the reactant side we have, sometimes let's say we had a molecule of A and a molecule of B. see that hump at the transition state? well that's the activation energy, that's the minimum amount of energy we need to get the reaction to go to the products. if we keep raise the temperature it increases the chance that A and B will collide successfully to form products.
certain reactions though if you keep increasing the temperature, instead of your reactants going to products, your products will go to reactants.
for example A + B Double arrow C + heat
You mean this way --> <--
this is an exothermic reaction, because heat is on the product side. like if we continued to raise the temperature here, the reaction will actually go the opposite way, the products will go back to the reactants to deal with that added heat.
@korosh23 yeah that's what I meant I don't think there's a button for that .
but generally yeah for all chemical reactions you need successful collisions, the key word here was "successful" hope this was helpful
Very helpful, thank you for your time. :)