Kinetics Flashcards
what is collision theory
particles must collide with enough energy at the right orientation
what does an increase in temperature have in chemical reactions
particles are faster as have more energy hence more collisions occur
what does an increase in concentration have in chemical reactions
more particles in given volume more collisions
what does an increase in pressure of gas have in chemical reactions
more molecules in a given volume hence more collisions
what does an increase in surface area have in chemical reactions
more area to react hence more sites=faster rate of reaction
what is the rate of reaction
the change in the amount of a reactant or product overtime
what is the calculation for rate of reaction
time
what is activation energy?
minimum energy required to start a reaction with successful collisions
what is a catalyst?
increases the rate of reaction by providing an alternative reaction pathway with a lower activation energy
how does a catalyst increase the rate of reaction on a maxwell boltzmann distribution
decreases the activation energy while moving the activation energy to the left so more molecules have the activation enrgy
how is the maxwell boltzmann distribution labled
x axis=kinetic energy
y axis=no.of molecules
top of peak=most probable energy
right of peak=is the average energy
how does temperature affect MBD
higher temperatures mean peak is lower and moves o the right, more particles with high energy
how does concentration effect MBD
increase the concentration means peak is higher more energies above the activation energy
how does increasing pressure effect MBD
raising pressure pushes all the gas particles closer together, increase the number of collisions
why at a fixed temperature, the rate of reaction doubles when the concentration doubles
double the amount of particles means twice the number of collisions in a given volume
