chapter 10 Flashcards
rate of reaction=
change in conc/ time
mol dm-3/s= mol dm-3 s-1
how does increasing the concentration affect ROR
- increase in conc increases the number of particles in the same volume, closer together- collide more frequently
- more effective collisions= faster ROR
how does increasing the pressure of a gas affect ROR
the concentration of the gas molecules increases, closer together and collide more frequently, leading to more effective collisions
catalyst
a substances that changes the ROR without undergoing any permanent change itself
-not used up
-may react with a reactant to form an intermediate or may provide a surface on which the reaction can take place
-at the end the catalyst is regenerated
provides an alternative reaction pathway of lower activation energy
homogeneous catalysts
& 2 examples
has the same physical state as the reactants
- reacts with the reactants to from an intermediate. the intermediate then breaks down to give the product and regenerates the catalyst
- making esters with a sulfuric acid catalyst
- ozone depletion- cl radicals as catalyst
heterogeneous catalysts
has a different physical state from the reactants, usually solid. reactant molecules are adsorbed onto the surface of the catalyst, after reaction the product molecules leave the surface of the catalyst by desorption
examples of heterogeneous catalysts
3
- Fe in harbour process
- Ni in hydrogenation of alkenes
- vanadium oxide in the contact process
features of the Boltzmann distribution
- curve starts at the origin- no molecules have zero energy
- the area under the curve is equal to the total number of molecules
- there is no maximum energy for a molecule- curve doesn’t meet the axis
Boltzmann distribution and temperature
at higher temp:
- more molecules have an energy greater than or equal to the activation energy
- greater proportion of collisions will lead to a reaction increasing the ROR
- collisions more frequent- moving faster
Boltzmann distribution and catalysts
a catalyst provides an alternative reaction route with a lower activation energy
- greater proportion of molecules have energy equal to or greater than the activation energy
in dynamic equilibrium
- the rate of the forward reaction is equal to the rate of the reverse reaction
- the concentrations of reactants and products do not change
le chatelier’s principal
states that when a system in equilibrium is subjected to an external change the system readjusts itself to minimise the effect of that change.
effect of concentration on equilibrium
A + B C + D
increase conc of A or B, decrease conc of C or
-left
effect of temp on equilibrium
- an increase in temperature shifts the equilibrium position in the endothermic direction
- decrease in temperature shifts the equilibrium position in the exothermic direction
effect of pressure on equilibrium
increasing the pressure of the system will shift the position of equilibrium to the side with fewer molecules, reducing the pressure