Question

Consider C₃H₈ (g) + 5 O₂ (g) à 3 CO₂ (g) + 4 H₂O (l), with the reaction being at equilibrium. ∆H^o = -2220 kJ.    What effect will increasing the temperature have on the system?

Answer 1

∆H^o given is -ve, that means the process is exo thermic or heat releasing.

If the temperature of the reaction is increased, the rate of the forward reaction decreases.

The equilibrium tends to move towards the left side, means reverse reaction becomes more favourable.

More specifically speaking, when the temperature of the system at equilibrium is increased, The increase in temperature corresponds to introducing heat into the system. This influx of heat pushes the system away from equilibrium and nature restores equilibrium by removing some of this additional heat. Because the reaction is exothermic, the reaction produces heat when it proceeds in the forward direction. Le Châtelier's Principle states that the system will react to remove the added heat, thus the reaction must proceed in the reverse direction, converting products back to reactants.