Could someone please check these definitions for me? :)

[Lols123]

Hey guys,

Got a SAC tomorrow on Reaction Rates so want to have my definitions fully correct as my teacher is a pretty harsh marker
Its just on the 4 different ways to increase reaction rates.

1) Temperature - Temperature is a measure of average kinetic energy. Hence by increasing it, we are able to increase the average kinetic energy of the particles reacting. This means that there will be a greater proportion of particles with energy levels higher than that of the activation energy allowing for a greater number of successful collisions, hence speeding up the reaction.

2) Concentration/Pressure - By increasing the concentration of reactants in solution and pressure of reactants as gases, we are able to increase the frequency of collisions as there will there will be a larger ratio of particles per unit of volume. Hence this increases the chance of successful collisions allowing for a faster reaction.

3) Adding a catalyst - By adding a catalyst, the reactants will adsorb onto the surface distorting the bonds between them so that are weakened/break, allowing for them to create bonds between each other much easier. This allows the reaction to complete much quicker. Hence it can be said that by adding a catalyst, it decreases the activation energy, providing an alternate reaction pathway in which there will be a greater number of particles with energy levels higher than that of the activation energy and hence a greater number of successful collisions.

4) Increasing Surface Area -By increasing the surface area, you are effectively increasing the exposed particles, enabling a higher frequency of collisions and thus a higher proportion of successful collisions.

Any Help is extremely appreciated.

[b^3]

Seems preety much right and well looks like a good set of revision notes, unless i have missed something.

[nacho]

omgwtf you guys have a SAC already?

[Lols123]

@b^3 thanks for that

@nacho lawl yeah think we have another one next week as well T.T
very depressing

btw anyone know a good definition for the collision theory?
Is it just "That a chemical reaction will only occur when particles collide with sufficient energy to overcome the activation energy barrier"?
Do I need to expand anymore?

[schnappy]

All right, but if you want to be super pedantic pressure and concentration are technically different. In chemistry and in terms of gases you can use them as the same, but pressure is the force applied to a surface by a gas, concentration is the amount/mass per volume. Of course with kinetic theory they're intrinsically related.