Kinetics Flashcards
What are the 3 conditions needed for a reaction to occur
- particles must collide in the correct orientation
- particles must collide with sufficient energy
- particles must collide
Factors that affect the rate of reaction
- temperature
- surface area
- concentration
- pressure
What are the different techniques used to measure rates of reactions
- change of colour (calorimetry)
- change in mass (scale)
- change in volume (gas syringe)
- change in concentration (titration)
Why does the rate of reaction decrease over time
the concentration of reactants decreases, thus the frequency of collisions decreases as well
Define activation energy
the minimum amount of energy needed for a reaction to occur
The effect of a catalyst on the activation energy
it provides the reactants with an alternative pathway which has a lower activation energy
The effect of increasing temperature on Maxwell-Boltzmann curve
more particles gain sufficient energy due to the increase in kinetic energy – more frequent and successful collisions
- the curve flattens and moves to the right
How to find the rate of a reaction at a specific time
draw a tangent line at the point
- calculate the gradient
How to find the average/overall rate of reaction using a graph
take max and min points
- calculate the gradient
How to find the order of a reaction
k [A]m [B]n
A= concentration
K= rate constant
m= order of the reaction
What does a reaction with order 0 mean + units
changing the concentration doesn’t have any effect on the rate of reaction
mol dm-3 s-1
What does a reaction with order 1 mean + units
changes in the concentration of reactants is directly proportional to the changes in the rate of reaction
s-1
What does a reaction with order 2 mean + units
changes in the concentration of reactants leads to an increase in the rate of reaction equal to the square of the change
mol-1 dm3 s-1
what is special about the rate constant
it is temperature dependent
- increasing the temperature will increase the value of the rate constant
What are the graphs for order 0, 1 and 2
concentration vs time
order 0: linear negative
order 1: negative exponential
order 2: even more negative exponential (steeper)