2SO\(_2\)(g) + O\(_2\)(g) ↔ 2SO\(_3\)(g)
ΔH = -189 kJ mol-1
The equilibrium constant for the reaction above is increased by?
-
decreasing the temperature of the system
- Increase the pressure of the system
- The addition of a catalyst to the system
- Increasing the surface area of the vessel
The correct answer is: A
Explanation
Decrease in temperature favors in Equilibrium Constant[k] for this exothermic reaction.
The only factor that can affect an equilibrium constant is temperature:
-
Endothermic reactions
Increasing the temperature increases the equilibrium constant, and decreasing the temperature decreases it.
-
Exothermic reactions
Increasing the temperature decreases the equilibrium constant, and decreasing the temperature increases it. - Option A
There is an explanation video available .