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affecting rates of reaction - Coggle Diagram
affecting rates of reaction
collision theory
for a chemical reaction to occur, the particles must collide with enough energy
the greater the frequency of successful collisions between reacting particles, the greater the rate of reaction.
activation energy
define:
the minimum amount of energy needed for a collision to be successful.
it is different for different reactants
for successful collisions to occur, particles must collide with energy equivalent or more to the activation energy
if the required energy is not met then the atoms will just bounce off each other and the reaction doesn't take place.
concentration
takes place in solution
higher the concentration of reactants in a solution,
the more number of reacting particles per unit volume
.
higher the concentration the higher the rate of the reaction.
pressure
takes place in gases
higher the pressure,
the closer together the reacting particles are
define rate:
a measure of how fast the reaction takes place
unit: cm^3/s
surface area
solid reactants
for a given mass of a solid,
powders or smaller lumps have larger surface area to volume ratios
than larger lumps.
bigger surface areas have grater exposed surface
particles collide more frequently, rate of reaction increases.
temperature
the higher the temperature, the particles gain more kinetic energy
reacting particles move more quickly
particles collide more frequently, greater rate of reaction in higher temperatures.
presence of catalyst