Topic C6 - The Rate And Extent Of Chemical Change Flashcards
How do you measure the mean rate of reaction?
Amount of product
formed
Mean rate of reaction= ————-
Time
What is Collision Frequency
The more collisions between particles, the faster the rate of reaction. Soy doubling frequency would double the rate
What is Collision energy
Enough energy need to be transferred in a collision to overcome the activation energy and break the bonds to start the reaction
How does temperature affect rates of reaction?
Higher temperature, faster particles move, more they collide, speed up reaction rate
How does pressure/ concentration affect rates of reaction
More particles in the same volume = more frequent collisions
How does surface area affect rates of reaction?
Small peices = fast rate, more particles or collide with
What is a reversible reaction?
Where the products can react to form the reactants again
When can equilibrium be reached
When a reversible reaction takes place IN A CLOSED SYSTEM!!
If the temperature increases, what direction does the equilibrium shift to?
Endothermic direction (to take in heat energy)
If the temperature decreases, what direction does the equilibrium shift to?
Exothermic (to release heat energy)
If the pressure increases, what direction does the equilibrium shift to?
Side with fewer molecule of gas
If the pressure decreases, what direction does the equilibrium shift to?
Side with more molecules
If the concentration of reactants INCREASES, what does the system do?
Make more products
If the concentration of the reactants DECREASES, what does the system do?
Make more reactants
Describe and explain effect of increasing concentration on rate of reaction
Concentration increases = faster reactio
More reactants = more frequent collisions
