Rate of Reaction Flashcards
What are the conditions for a reaction to take place?
- particles must collide
- must have enough energy to react
What is the effect of…
- concentration
- pressure
on the rate of reaction?
- increase in concentration = increase in rate
- increase in pressure = increase in rate
because both result in more particles in a given volume so more collisions occur
Boltzmann Distribution
- no molecules have zero energy
- straight line flattens to peak
- exponential curve
activation energy
What are its units?
minimum energy needed for a collision to be successful and a reaction to take place
(kjmol -1)
What is the effect of temperature on the rate of reaction?
at T1 - distribution shows how many particles have a minimum energy for activation energy
at T2 - mean energy of particles increases (larger area shaded shows more particles have activation energy, more collisions successful so rate is faster
catalyst
- substance that increases the rate of reaction without itself being used up by providing an alternate route for the reaction that has a lower activation energy
- lower activation energy ensures that more particles will have it
- more collisions successful, rate will increase
What are the different types of catalyst?
- homogenous catalyst
- heterogenous catalyst
- homogenous catalyst
- heterogenous catalyst
- catalyst and the reactants are both present in the same phase (e.g. both liquid)
- catalyst and reactants present in different phases
rate of reaction
change in concentration of reactants per unit time
rate of reaction equation
delta[] / delta t
How to find the rate of reaction from a graph?
find tangent at that point
What is the effect of surface area on rate of reaction?
increase surface area = increase rate
greater frequency of collisions
more successful collisions per second
What are the units of rate of reaction?
moldm-3s-1
