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Flashcards in 2. Equilibria Deck (12):
1

Fastors that effwect rate?

catalyst.
pressure
concentration
surface area
temperature

2

What is rate of reaction?

rate= change in concentration/time.

3

Catalys examples?

iron in the haber process.
vanadium (5) oxide in the contact process.
Ni in hydration of margarine.

4

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.

5

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.

6

what is a homogeneous catalyst?

in the same physical state as the reactants.

7

what is a heterogeneous catalyst?

in a different state to the reactants.

8

Define dynamic equilibrium.

the equilibrium that exists in a closed system when the rate of the forward reaction = rate of the backwards reaction.

9

Where are catalyst naturally found?

as enzymes.

10

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.

11

2 uses of enzymes as a catalyst.

fermentation
washing powders.

12

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.