Yet another reaction has an equilibrium constant kc=4.32×105 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? the equilibrium constant will yet another reaction has an equilibrium constant at 25 . it is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. if the temperature is raised to 200 , what will happen to the equilibrium constant?

The equilibrium constant will decrease.
when this reaction is an exothermic reaction, SO we can assume heat as a product of that reaction.

when Kc = concentration of product/concentration of reactants

So when the temperature and heat increase the reaction will go in the direction which decreases the heat and achieves equilibrium again. So it will go leftwards to decrease the products. and when the products decrease the Kc will decrease. 

The equilibrium constant will decrease

Explanation:
The equilibriuc constant (Kc) can be calculated as follows:
Kc = 

Now, the given equation is an exothermic reaction. This means that heat is s product.

If we increase the amount of heat, the system will no longer be at equilibrium. This equilibrium will shift to the left creating more reactants in order to balance the system and be reach equilibrium again.

By this, we can note that the concentration of reactants in the system will increase which means that the equilibrium constant will decrease.

Hope this helps :)

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