669377
Description
Mind Map by wondersnail, updated more than 1 year ago
|
Created by wondersnail
over 10 years ago
|
|
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
Want to create your own Mind Maps for free with GoConqr? Learn more.