Questions: Yet another reaction has an equilibrium constant Kc=4.32 x 10^5 at 25°C. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. If the temperature is raised to 200°C, what will happen to the equilibrium constant?

Yet another reaction has an equilibrium constant Kc=4.32 x 10^5 at 25°C. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. If the temperature is raised to 200°C, what will happen to the equilibrium constant?

Transcript text: Yet another reaction has an equilibrium constant $K_{c}=4.32 \times 10^{5}$ at $25^{\circ} \mathrm{C}$. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. If the temperature is raised to $200{ }^{\circ} \mathrm{C}$, what will happen to the equilibrium constant?

Solution

Solution Steps

Step 1: Understand the Effect of Temperature on Equilibrium Constant

For an exothermic reaction, increasing the temperature generally shifts the equilibrium position to favor the reactants. This is because adding heat to an exothermic reaction is akin to adding a product (heat), which according to Le Chatelier's principle, will shift the equilibrium to the left (towards the reactants).

Step 2: Apply Le Chatelier's Principle

Since the reaction is exothermic, raising the temperature will decrease the equilibrium constant $ K_c $. This is because the equilibrium shifts towards the reactants, reducing the concentration of products relative to reactants at equilibrium.