What happens to the equlibrium constant if the pressure increased?
the Kc of 2NH3<=>N2+3H2 is 0.03
N2 is (0.1M)
H2 is (0.3M)
NH2 is (1M)
The equilibrium constant is just that, a constant, and is not subject to change with pressure changes. It will change with temperature changes.
To explain why the equilibrium constant does not change with pressure changes, let's first understand how pressure affects the equilibrium of a reaction.
According to Le Chatelier's principle, when an external stress is applied to a system in equilibrium, the system responds by shifting in a direction that counteracts the stress to reach a new equilibrium. In the case of pressure changes, the system will shift towards the side of the reaction with fewer gas molecules if the pressure increases, or towards the side with more gas molecules if the pressure decreases.
Now, let's apply this principle to the equation 2NH3 ↔ N2 + 3H2. In this reaction, we have four moles of gas molecules on the left side (2NH3) and four moles of gas molecules on the right side (N2 + 3H2). Therefore, any change in pressure would not affect the equilibrium position because the system is not being stressed by a change in the number of gas molecules.
So, in summary, changes in pressure will not alter the value of the equilibrium constant (Kc) for a reaction involving only gaseous substances, as long as the number of gas molecules remains the same.
Regarding the given values in the problem, the equilibrium constant (Kc) of 0.03 remains unchanged even if the pressure increases or any of the concentrations (N2, H2, NH3) change.