For the reaction H2 (g) + I2 (g) ⇋ 2HI(g)the equilibrium constant Kp changes with
For the reaction H2 (g) + I2 (g) ⇋ 2HI(g)the equilibrium constant Kp changes with
the amounts of 
and 
present
The correct option is D temperature
Always remember: When we talk about a "particular” equilibrium, we uniquely identify it by a temperature. Unless otherwise specified, the temperature does not change.
Characteristics of equilibrium constant (Kp)
1.For a given reaction, the value of the equilibrium constant depends only on the temperature.
2.It is independent of the direction from which the equilibrium is attained or the initial concentrations of the reacting species
3.It is independent of Volume or the presence of catalysts
4.Kp does not change due to the presence of inert gases
All these shall be applicable for the other equilibrium constant Kc as well. The difference between the two is the way in which the "active mass” is expressed. If we use molar concentrations then we are utilizing Kc. On the other hand, if we use partial pressures, then Kp is implied. Other active masses like mole fractions might also be used to derive a new form of equilibrium constant.
temperature
Always remember: When we talk about a "particular” equilibrium, we uniquely identify it by a temperature. Unless otherwise specified, the temperature does not change.
Characteristics of equilibrium constant (Kp)
1.For a given reaction, the value of the equilibrium constant depends only on the temperature.
2.It is independent of the direction from which the equilibrium is attained or the initial concentrations of the reacting species
3.It is independent of Volume or the presence of catalysts
4.Kp does not change due to the presence of inert gases
All these shall be applicable for the other equilibrium constant Kc as well. The difference between the two is the way in which the "active mass” is expressed. If we use molar concentrations then we are utilizing Kc. On the other hand, if we use partial pressures, then Kp is implied. Other active masses like mole fractions might also be used to derive a new form of equilibrium constant.
