Equilibrium Shift
Let a reversible gas reaction settle into equilibrium, then disturb it — add a reactant, remove product, compress or expand the vessel, or heat or cool it — and watch the concentrations shift and resettle into a new equilibrium, with a visible colour change for the nitrogen dioxide reaction.
What you can adjust
- Reaction
- 0 – 1
- Temperature
- 260 – 340 K
- Initial [reactant A]
- 0 – 1 mol/L
- Initial [reactant B]
- 0 – 1 mol/L
- Initial [product]
- 0 – 1 mol/L
- Disturbance
- 0 – 7
- Disturbance time
- 1 – 8 s
Which reversible gas-phase reaction to run.
Starting temperature. 298 K (~25 degC) is the reference temperature the equilibrium constant is quoted at.
Starting concentration of the first reactant (NO2, or N2 for the Haber reaction).
Starting concentration of the second reactant. Only used by the N2 + 3 H2 <=> 2 NH3 reaction (H2) — ignored for 2 NO2 <=> N2O4, which has only one reactant.
Starting concentration of the product (N2O4, or NH3 for the Haber reaction).
What disturbs the equilibrium partway through the run. 'Add inert gas' is the case everyone gets wrong — at constant volume it changes nothing, because it changes no reacting species' concentration.
When (in seconds) the disturbance is applied. The reaction is given this long to reach its initial equilibrium first.