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...affect the equilibrium p? Le Châtelier’s principle is stated (Section 13.7) as follows: “If a
change is imposed on a system at equilibrium, the position of
the equilibrium will shift in a direction that tends to reduce that
change.” The system N2 +3H2 <--> 2NH3 is used as an example
in which the addition of nitrogen gas at equilibrium results
in a decrease in H2 concentration and an increase in NH3 concentration.
In the experiment the volume is assumed to be constant.
On the other hand, if N2 is added to the reaction system in a
container with a piston so that the pressure can be held constant,
the amount of NH3 actually could decrease and the concentration
of H2 would increase as equilibrium is reestablished. Explain
how this can happen. Also, if you consider this same system at
equilibrium, the addition of an inert gas, holding the pressure
constant, does affect the equilibrium position. Explain why the
addition of an inert gas to this system in a rigid container does
not affect the equilibrium position.
change is imposed on a system at equilibrium, the position of
the equilibrium will shift in a direction that tends to reduce that
change.” The system N2 +3H2 <--> 2NH3 is used as an example
in which the addition of nitrogen gas at equilibrium results
in a decrease in H2 concentration and an increase in NH3 concentration.
In the experiment the volume is assumed to be constant.
On the other hand, if N2 is added to the reaction system in a
container with a piston so that the pressure can be held constant,
the amount of NH3 actually could decrease and the concentration
of H2 would increase as equilibrium is reestablished. Explain
how this can happen. Also, if you consider this same system at
equilibrium, the addition of an inert gas, holding the pressure
constant, does affect the equilibrium position. Explain why the
addition of an inert gas to this system in a rigid container does
not affect the equilibrium position.