Can successful collision in collision theory be used for a solid metal and an (aq) substance?
Ex. Fe(s) + 2HCl (aq) --> H2(g) + FeCl2 (aq)
Stacey Warren - Expert brainly.com
Hey! We 've verified this expert answer for you, click below to unlock the details :)
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga.
Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus.
Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
If yes, by increasing the temperature, do I increase the successful collisions right?
Not the answer you are looking for? Search for more explanations.
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
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.
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