Kinetics Flashcards
What must particles do in order to react?
Collide with sufficient energy (activation energy)
Do most collisions result in a reaction?
No
Define activation energy?
The minimum energy that particles must collide with for a reaction to occur
Why is the effect of increasing temperature on the rate of reaction? Why?
Increasing temperature -> increased rate of reaction
Much higher proportion of particles have energy greater then the activation energy -> many more successful collisions per second -> increased rate
What is the effect of increasing concentrations/ pressure on the rate of reaction? Why?
Increased concentration/ pressure -> increased rate of reaction
There are more particles in a given volume -> more frequent successful collisions -> increased rate
What is a catalyst?
A substance which increaSes the rate of reaction by providing an alternative pathway but is not used up in the reaction
How do catalysts work and how do they increase the rate of reaction?
Provide an alternative reaction pathway (one with a lower activation energy)
Lowers activation energy, so more particles have energy> activation energy, so more frequent successful collisions, so increased reaction rate
Why does the curve of a maxwell Boltzmann curve start at the origin?
No molecules have no/zero energy
What is the dotted line found on the energy plane
Most probable energy
give a correct statement about a sample of gas molecules
At a given temperature, the average kinetic energy is constant
