Kinetics Flashcards
Define reaction rate:
It is the change in concentration of reactant or product over time.
How do you work out reaction rate?
Amount of reactant used or product formed/time
What is the collision theory?
- Particles must be colliding in the right direction and facing the right way.
- Particles must have minima amount of kinetic energy in order to collide.
Define activation energy:
The minimum amount of kinetic energy that particles need to react.
How does increasing temperature affect reactions?
- The particle move faster so greater proportion of molecules have at lease the activation energy and able to react which pushes the Maxwell Boltzmann distribution to the right. The particles collide more often.
How does increasing the concentration increase the rate of reaction?
If you increase concentration the particles will move closer together so will collide more often and more frequent collisions so they’ll have more chance to react increasing the reaction rate.
How does increasing the pressure increase the rate of reaction?
If you raise pressure the gas particles will move closer together so will collide more often and more frequent collisions so they’ll have more chance to react increasing the reaction rate.
What are catalysts?
A catalyst is a substance that increases the rate of reaction by lowering activation energy and providing alternative reaction pathway without being used up in the end. Produce products faster at a lower temperature.
How do catalysts increase the rate of reaction?
The catalysts lowers the activation energy so more particles with enough energy are able to react and using a different route so more particles can react. This moves the activation energy to the left.
Define reversible reactions:
Reactions are reversible so go both ways.
What is dynamic equilibria?
When forward and backward reactions are happening at the same and constant rate in a closed system,
How does concentration affect equilibrium?
- If increasing the concentration of reactants the equilibrium gets rid of extra reactants by producing more products so equilibria shifts to the right.
- If increasing the concentration of products the equilibrium gets rid of extra products by producing more reactants so equilibria shifts to the left.
How does pressure affect equilibrium?
- Increasing the pressure moves equilibria to the side and there is fewer gas molecules and reduce in pressure.
- Decreasing the pressure moves equilibria to the side and there is an increase in gas molecules and a raise in pressure.
How does temperature affect equilibrium?
- Increasing temperature increases heat so equilibria moves in endothermic way.
- Decreasing temperature means removing heat so equilibrium moves in exothermic way producing more heat.
Do catalysts affect the position of equilibrium?
No they cannot increase yield but can allow equilibrium to be reached faster.
