Chapter Five : Rates of Reactions Flashcards
Collision Theory
States that a chemical reaction has particles that are moving in random motion and the rate of successful collisions give the rate of reaction
Collision Theory reaction requirements
Reactants must;
Collide
Have correct orientation to break bonds
Have sufficient energy for reactants to occur
How are reaction rates observed
Volume of gas evolved Mass of a solid formed Decrease in mass Intensity of colour Formation of a precipitate pH Temperature
Maxwell-Boltzmann distribution curves
Statistical range of energies present in particles of a gas sample
Number of particles with a particular energy graphed against the energy
Shows the velocities of particles
Highest part represents most probable velocity
Factors that affect rate of reaction
Concentration Pressure Temp Catalysts Surface Area
Effect of concentration on rate of reaction
When concentration is increased there are more particles to bounce off each other increasing rate of successful collisions
Effect of pressure on rate of reaction
When pressure is increased the particles increase their rate of successful collisions
Effect of temp on rate of reaction
Increases the amount of particles with high energy, more particles have enough energy to break bonds
Also increases frequecy of collisions due to faster moving particles
Catalyst effect on rate of reaction
Provides an alternative reaction pathway with a lower activation energy
It allows particles with less energy to break the bonds of reactants
Surface area effect on rate of reaction
Increasing surface area means that more reactant particles can collide with one another and therefore there are more successful collisions