How does a temperature change differ from a concentration change in its effect on an equilibrium?

1. Changing a concentration moves the reaction quotient away from a fixed constant. 2. The system then shifts until the quotient returns to that same unchanged constant. 3. Changing the temperature is different, because the constant itself takes a new value. 4. The direction of the resulting shift can still be predicted by treating heat as a stress. 5. Temperature effects are not confined to gases, since solution equilibria respond too. 6. The position certainly does move, so calling it unmoved contradicts the observation. _Source: OpenStax Chemistry (CC BY 4.0), Ch 13 "Fundamental Equilibrium Concepts", section 13.3 Shifting Equilibria: Le Châtelier's Principle_