For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium const

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?

Step 1: Identify the type of reaction. The given reaction is N2(g) + 3H2(g) ⇌ 2NH3(g). This reaction is exothermic, meaning it releases heat.
Step 2: Understand what happens when temperature increases. For exothermic reactions, increasing the temperature adds heat to the system.
Step 3: Apply Le Chatelier's Principle. According to this principle, if you add heat to an exothermic reaction, the equilibrium will shift to the left to absorb the extra heat.
Step 4: Determine the effect on the equilibrium constant. When the equilibrium shifts to the left, the concentration of reactants increases and the concentration of products decreases, which results in a decrease in the equilibrium constant.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Exothermic vs. Endothermic Reactions – Understanding the nature of the reaction (whether it releases or absorbs heat) is crucial for predicting the effect of temperature changes on equilibrium.
Equilibrium Constant (K) – The equilibrium constant is a value that expresses the ratio of the concentrations of products to reactants at equilibrium, and it is temperature-dependent.