Why, when temperature is increased, does the position of equilibrium shift to RIGHT for this reaction?
Colourless: N2O4(g) ↔ Brown: 2NO2(g) ΔH = + 54kjmol-1
Forward reaction is endothermic, thus reducing the temp
Forward reaction is exothermic, thus reducing the temp
Forward reaction is endothermic, thus increasing the temp
Forward reaction is exothermic, thus increasing the temp
The correct answer is "Forward reaction is endothermic, thus increasing the temp".
This is because the forward reaction (N2O4(g) → 2NO2(g)) is endothermic, meaning it absorbs heat as the reaction proceeds. Increasing the temperature will introduce more heat into the system, which will help to compensate for the energy absorbed during the forward reaction. This means that the reaction will proceed more readily in the forward direction, causing the position of equilibrium to shift to the right towards the product side (2NO2(g)).