Kinetics ( AS ) Flashcards
What must particles do in order to react?
Collide with sufficient energy(activation energy) and correct orientation
Do most collisions result in a reaction?
No
Define activation energy
The minimum amount of energy that particles must collide with for a reaction to occur
What does the maxwell boltzmann distribution show?
The spread of energies that molecules of a gas or liquid have at a particular temperature
Why should the energy distribution go through the origin?
There are no molecules with no energy
Where is the Emp line on the graph?
From the peak down to the X-Axis
What does the area under the curve represent?
The total number of particles present
Why should the energy distribution never meet the X-axis?
Because there is no maximum energy for molecules
What’s the label for the y-axis?
Number of molecules
Whats the label for the X-axis?
Energy
What is the effect of increasing temperature on the rate of reaction?why?
Increasing temperature—>increased rate of reaction
More particles have energy that’s greater than activation energy—> increased frequency of successful Collisions
What happens to the peak of the maxwell boltzmann distribution when the temperature is increased?
It moves to a higher energy with a lower height
What is the effect of increasing concentration/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
Will the area under the curve differ when the concentration is increased?
Yes, because there are more particles, meaning the peak will be higher
What is a catalyst?
A substance that increases the rate of reaction but is not used up in the reaction
