For a reaction at equilibrium, if the temperature is increased and ΔH is positiv

For a reaction at equilibrium, if the temperature is increased and ΔH is positive, what will happen to the position of equilibrium?

For a reaction at equilibrium, if the temperature is increased and ΔH is positive, what will happen to the position of equilibrium?

Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the forward and reverse reactions occur at the same rate.
Step 2: Know that ΔH (delta H) represents the change in enthalpy, or heat content, of the reaction. A positive ΔH means the reaction absorbs heat (endothermic).
Step 3: Remember Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 4: Recognize that increasing the temperature adds heat to the system.
Step 5: Since the reaction is endothermic (ΔH is positive), the system will shift to the right to absorb the added heat.
Step 6: Conclude that the position of equilibrium will shift to favor the products of the reaction.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Endothermic vs Exothermic Reactions – Understanding the difference between endothermic (absorbing heat) and exothermic (releasing heat) reactions is crucial for predicting the direction of the shift in equilibrium.