kinetics 3.1.5 in papers 2 + 3
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define the rate of reaction
• change in amount of a reactant or product in a given time period
define collision theory.
• a collision between particles needs to have sufficent energy for a reaction to occur
define activation energy.
• the minimum energy reacting particles require for successful collision
what factors affect the rate of reaction?
• pressure ofmgas • tempreture • concentration of a solution • catalyst
what effect does an increase in tempreture have on the intial rate of reaction and final volume?
• initial rate = increase • final volume = no effect
what effect does an increase in concentration have on the intial rate of reaction and final volume?
initial rate = increase final volume = increases if its the limiting reagent
what effect does an increase in surface area have on the intial rate of reaction and final volume?
initial rate = increase final volume = no effect
what effect does an increase in surface area have on the intial rate of reaction and final volume?
initial rate = increase final volume = no effect
what effect does adding a catalyst have on the intial rate of reaction and final volume?
inital rate = increase final volume = no effect
why does a maxwell boltzmann curve go through the origin?
no particles have no energy
what does asymptotically mean?
doesnt touch the x-axis, particles have an infinite amount of energy
what does the area under the curve mean?
total number of particles
what is the maximum energy?
there isnt one
whats the most probable energy?
the most common energy under the peak
where is the mean energy?
right hand side of the graph/lower part
what happens when we increase tempreture on a boltmann curve?
• reaction increases • particles have more kenetic energy and move faster • so greater amount of molecules will have energy equal to or greater than activation energy and therefore increase the rates of successful collisions • graphs peak is lower and shifts to the right
what effect does a catalyst have on boltzmann curve?
• increases rate of reaction by providing an alternative route with lower activation energy • it remains chemically unchanged and is regenerated
what effect does pressure have on the boltzmann curve?
• lower pressure = lower peaker peak • less numbers of particles with energy equal to or more than activation energy