As pressure rises, the equilibrium will move to the side of the reaction where there are less moles of gas. When the pressure drops, the equilibrium will move to the side of the process where there are more gas molecules.
Similar to how concentration has no bearing on Kc's value, pressure has no impact on Kp's.
As a result of the equilibrium shifting in favour of the direction with fewer moles due to an increase in pressure, the pressure falls.
Kp is unchanged because the reactant to product partial pressure ratio remains constant.
According to Charles' law, a gas's volume will double if its temperature doubles.
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