Arrhenius Equation (A-level IB Chemistry)

[@106four]

This video is a gem!! Perfect explanation, flawless editing, very very underrated

[@chemistry.student]

Thank you!

[@abu-karz]

​@@chemistry.student Is the arrhenius equation applicable for all reactions? What about in cases solid phase reactions where it's not concentration...

[@maximecassart79]

Hello, I love your videos so much keep up the good work. Also, I have a question why did you consider k as a portion of particles from [x][y]? I thought [x][y] were the concentration of products formed or consumed thus all there particles had surpassed the activation energy and collided with the proper orientation as opposed to a portion as mentioned in the video. May you please clarify? Sorry if this question does not make sense.

[@chemistry.student]

Remember the rate constant is related to the rate of the reaction - how many successful collisions are occurring per second, it has nothing to do with the total amount of product formed and therefore final concentrations of product. Only a tiny fraction of reactant particles will collide with the required activation energy and orientation in the first second. The rate consant k is linked to this fraction (proportion) of reactant particles. Hope that helps :)

[@abu-karz]

Is the arrhenius equation applicable for all reactions? What about in cases solid phase reactions where it's not concentration...

[@chemistry.student]

Good question! In short, no, the Arrhenius equation doesn't work in some scenarios (including solid-phase reactions). It is primarily used for modelling gas-phase and solution-phase reactions where concentration change is a primary factor in determining rate due to particle collisions. It can be still be useful for other reactions, however additional modelling and modifications would be required.

[@s4ltw0rm]

Thank you

[@chemistry.student]

Thank you - hope it helped :)