: 200
Concentration change: Adding reactant shifts right; adding product shifts left. Removing a species shifts toward the removed side. K unchanged. Pressure change (gases only): Increasing pressure shifts toward fewer moles of gas; decreasing pressure shifts toward more moles. K unchanged. For reactions with delta_n_{gas} = 0, pressure has no effect. Inert gas at constant volume: No effect (partial pressures unchanged). Inert gas at constant pressure: Volume expands; shifts toward more gas moles. Temperature change: Increasing T shifts toward endothermic direction. This is the ONLY change that alters K. For exothermic: K decreases. For endothermic: K increases. Catalyst: No effect on K or equilibrium position. Speeds attainment of equilibrium. Volume change: Halving volume doubles pressure — same as pressure increase. Doubling volume halves pressure. Removing product continuously: Shifts right indefinitely (no equilibrium reached). This is used industrially in Haber process and Contact process.