Reaction rates Flashcards
what is the rate of reaction
the change of conc/amount of a reactant or product per unit time
what is the calculation for rate
amount of reaction used or product made/ time
explain collision theory
for a reaction to occur particles must collide in the right direction nd have the minimum amount of kinetic energy
what is the minimum amount of energy required for a reaction to occur called
activation energy
draw a labelled energy profile diagram
reactions that have a low activation energy need _____ energy to break the bonds
less
draw a labelled Boltzmann graph
how does temperature affect a Boltzmann graph
curve shifts right
peak is lower
area under curve us the same
area under curve beyond activation area increases
why does increased temp lead to increased rate
particles have more kinetic energy
therefore increased chnaces of successful collisions
why does increasing pressure increase rate
particles are closer together so more frequent collisions and higher chance of reaction
how does a catalyst increase rate of reaction
provide alternative reaction pathway that has a lower activation energy, remains unchanged in reaction
what is a heterogeneous catalyst and give an example
catalyst in a different state to reactants
solid iron catalyst used in Haber process
increasing the _____ ____ of the heterogenous catalyst will increase the rate of the reaction
surface area
what is a homogenous catalyst
catalyst in same state to reactants
sulphuric acid to make an ester
they are used up landform intermediate species by combining with reactants to form products
catalyst is then reformed
why are catalyst used in industry, give an example
low temperatures- less money spent and less CO2 produced
speed up
change properties of a product
benefits environment
less waste as better atom economies
catalytic converters I cars reduce levels of pollution
