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Kinetics
AQA A Level Chemistry
| Question | Answer |
|---|---|
| What does collision theory state? | For a reaction to take place particles must collide AND they must collide with enough energy to break the bonds in the reactants |
| How does increasing temperature increase the rate of reaction? | This increases the kinetic energy of particles, this increases the frequency and energy of collisions |
| How does increasing concentration increase the rate of a reaction? | There are more particles in a given volume, so they are closer together, resulting in more frequent collisions |
| How does increasing the pressure of a gas increase the rate of a reaction? | There are more particles in a given volume, so they are closer together, resulting in more frequent collisions |
| How does increasing the surface area of a solid increase the rate of reaction? | More particles are exposed and are available to collide, resulting in more frequent collisions |
| How does a catalyst increase the rate of a reaction? | Catalysts provide an alternative pathway with a lower activation energy - this means more particles have the minimum energy for successful collisions to occur |
| What is activation energy | The minimum amount of energy required to break the bonds in the reactants to allow the reaction to occur |
| What is along the x and y axes in a Maxwell Boltzmann distribution graph? | x-energy, y-fraction of particles |
| Sketch a typical Maxwell Boltzman distribution curve and indicate the average + most probable energy | Draw |
| Why does the Maxwell Boltzmann curve start at zero? | No particles have zero energy |
| Why does the right hand side of the curve ever touch the axid at zero | There are no upper limit to the amount of energy some particles may have |
| What does the area under a Maxwell Boltzmann curve correlate to? | The total number of particles |
| Sketch a typical Maxwell Boltzman distribution curve and another at a higher temperature | Draw |
| What does the area under a Maxwell Boltzman curve at and above Eact represent? | The number of particles that have at least the activation energy and above to react |
| What happens to the number of particles with Eact and above at higher temperatures? | Increases |
| What happens to Eact when a catalyst is used? | The Eact with a catalysts is lower, which results in more particles having the minimum energy in order to react successfully |
Created by:
JBearfield
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