669377
Descrição
Mapa Mental por wondersnail, atualizado more than 1 year ago
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Criado por wondersnail
mais de 10 anos atrás
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7.2 - The Position of Equilibrium
- Equilibrium Constant, Kc -
has a fixed value for a
particular reactions at a
specified temperature.
Can only be changed for a
reaction by adjusting the
temperature
- Calculated from the
equilibrium concentrations.
Products divided by
reactants, raised to their
coefficients.
- The higher magnitude of Kc,
the further a reaction has
gone, i.e. the more products
there are compared to
reactants.
- For example, if Kc < 0,01,
the eqm concentration of
reactants is considered to
be equal to their initial
concentrations, since the
forward reaction almost
does not happen
- For example, if Kc < 0,01,
the eqm concentration of
reactants is considered to
be equal to their initial
concentrations, since the
forward reaction almost
does not happen
- Le Chatelier's Principle- When a
system at equilibrium is subjected to
change, it will respond in such way as
to minimise the effect of the change
- Increaseing the concentration of a reactant:
equilibrium shifts to the right
- Decreasing the concentration of reactant:
equilibrium shifts to the left
- Increasing the pressure: shifts
toward the side with the least
number of gaseous molecules
- Drecreasing the pressure: shifts
towards the side with the most
number of gaseous molecules
- Increasing the temperature:
shifts towards the side with
endothermin products
- Increases Kc
- Increases Kc
- Decreasing the temperature:
shifts towards the side with
exothermic products
- Decreases Kc
- Decreases Kc
- Adding a catalyst does not shift
the equilibrium; it increases the
rate of both forward and backward
reaction
- Increaseing the concentration of a reactant:
equilibrium shifts to the right
- Haber process
- 1Nitrogen and 3hydrogen
creates 2ammonia
- Exothermic reaction
- Iron acting as a catalyst
- 1Nitrogen and 3hydrogen
creates 2ammonia
- Contact process
- 1sulphur and 1 oxygen
creates sulphur dioxide, which
is oxidised into sulphur
trioxide, which is combined
with water to create sulphuric
acid
- Second step is the rate-determining step
- Exothermic rate-determining step
- V2O5 as catalyst
- 1sulphur and 1 oxygen
creates sulphur dioxide, which
is oxidised into sulphur
trioxide, which is combined
with water to create sulphuric
acid
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