Final answer:
Increasing the temperature of the equilibrium system 2CO(g) + C(s) ⇌ CO₂(g) will cause the equilibrium to shift to the left, as this is an exothermic reaction and the system reacts to absorb the added heat according to Le Chatelier's Principle.
Step-by-step explanation:
For the equilibrium reaction 2CO(g) + C(s) ⇌ CO₂(g) + heat, when the temperature increases, the equilibrium will shift to the left. This happens because increasing the temperature adds energy to the system, and according to Le Chatelier's Principle, the system will shift towards the direction that absorbs the added energy. In this reaction, heat is produced in the forward reaction, so the system will shift to the left, which is the endothermic direction, to absorb the excess heat.
As for the effects of changing the temperature on other equilibrium systems, generally, if the reaction is exothermic (releases heat), increasing the temperature will shift the equilibrium towards the reactants. If the reaction is endothermic (absorbs heat), increasing the temperature will shift the equilibrium towards the products. These changes occur as the equilibrium constant is temperature dependent.