2. Equilibria
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Fastors that effwect rate?
catalyst. pressure concentration surface area temperature
What is rate of reaction?
rate= change in concentration/time.
Catalys examples?
iron in the haber process. vanadium (5) oxide in the contact process. Ni in hydration of margarine.
Define catalyse.
speeds up rate by providing an alternate reaction pathway with a lower activation energy. isnt used up in the reaction. may form an intermediate.
Economic importance of catalysts?
made more quickly and easily. requiring less energy- cuts fuel cost. reduces waster as a different reaction may now be possible which have better % yield and atom economy.
what is a homogeneous catalyst?
in the same physical state as the reactants.
what is a heterogeneous catalyst?
in a different state to the reactants.
Define dynamic equilibrium.
the equilibrium that exists in a closed system when the rate of the forward reaction = rate of the backwards reaction.
Where are catalyst naturally found?
as enzymes.
Why use enzymes in industry?
lower temps and pressures can be used. usually pure products are formed- so no separation is needed. Are biodegradable (other ones are toxic) so are easy to dispose.
2 uses of enzymes as a catalyst.
fermentation washing powders.
what is le chateliers principle?
that when a system is in dynamic equilibrium and is subject to a change, the equilibrium position will shift to minisise it.