10.2 catalysts module 3 Flashcards
what is a catalyst?
substance that changes the rate of reaction by providing an alternative pathway with lower activation energy without undergoing any permanent change itself
how does a catalyst react with the reactants?
may react with a reactant to form an intermediate or may provide a surface for the reaction to take place on
what happens to the catalyst at the end of the reaction?
it is regenerated
what is a homogenous catalyst?
same physical state as the reactants
what is a heterogenous catalyst?
different physical state from the reactants
how do the reactant molecules react on the surface of the catalyst?
they are adsorbed onto it
what does adsorb mean?
weakly bonded
what happens to the catalyst after it has been adsorbed and the reaction has ended?
desorption of the catalyst
what percentage of chemical materials are made using a catalyst?
estimated 90%
how is using a catalyst more sustainable for industry work?
lower activation energy means lower temperature needed and lower energy requirements so less electricity or fossil fuels are used
product is also made faster so costs less money and makes more money
reduces use of toxic solvents
what does sustainability require?
industry to operate processes with high atom economies and fewer pollutants
what is a catalyst used in industry and for what process?
Haber process
N2(g)+ 3H2(g) reversible reaction 2NH3(g)
catalyst= solid iron
