unit 4 - rate of reaction Flashcards
collision theory
for a sucessfull reaction, particles must collide with sufficient energy in the corrent orientation
activation energy
Min. amount of energy required by reacting materials to break down existing bonds and form new ones
to increase rate of reaction 2 simplest things to do?
more frequent collision
more successful collisions
how to measure activation enegry?
difference between the activation complex and reactants energy
how to achieve more frequenct collisions?
increase particle speed or increase particles present
how to acheieve more successful collisions?
give particle more energy or lower activation energy
how to calculate rate of reaction
Amount of reactant used/time
or
Amount of product formed/time
A steeper curve in the reaction graph indicates
a faster rate of reaction
whose concentration increases and decreases in a reaction?
concentration of reactants decrease, concentration of products increase
why do reactions slow down after some times
fewer reactants left to collide with
Increase surface area in ror
increases chance of collisions which means more particles are exposed
Powdered solids react quicker than larger lumps
Increase temp in ror
Particles get more energy and reach activation energy faster
Particle speed increases
Adding a catalyst in ror
Provide an alternate pathway to travel with less activation energy
Catalyst remain unchanged both physically and chemically
Why are catalysts widely used in the real world
Allow reaction to take place at lower temp
Saves energy
Have great economic importance in production
Are often enzymes
Can reduce pollution
Increasing concentration of solution in ror
Results in more frequenct collisions
Low concentrasion = low collisions = slow ror
High concentration = high collisions = fast ror
