5 posts • Page 1 of 1
Hi I'm still a little unclear as to why an inert gas will not effect the equilibrium constant despite increasing the pressure (when the volume is constant), and was wondering if someone could please explain the concept behind that. Thank you.
The inert gas doesn't react with the reactants and products that are at equilibrium. As a result, the concentration of the products and reactants is still the same and the K value is constant.
Pressure, even when volume is changed, will not change your equilibrium constant, K. Temperature is the only physical parameter that can change K, concentration and pressure can shift the direction to which the equilibrium will go towards, but they will not change K.
The only factor that can change the equilibrium constant is temperature. Pressure can not change Equilibrium constant but it changes the direction of the reaction only if the change in pressure was caused by a change in volume because in that case there was a change in concentration.
Who is online
Users browsing this forum: No registered users and 1 guest