At constant temperature, the equilibrium constant `(K_(p))` for the decomposition reaction
`N_(2)O_(4) hArr 2NO_(2)`
is expressed by `K_(p)=4x^(2)p//(1-x^(2))`, where p=pressure x= extent of decomposition. Which of the following statements is true?

Options

A. `K_(p)` increases with increase in p.
B. `K_(p)` increases with increase in x.
C. `K_(p)` increases with decrease in x.
D. `K_(p)` remains constant with change in p and x

Answer

D

Explanation

The equilibrium constant does not change at all with changes in concentrations, volume, pressure and presence of catalyst. It changes only with changes in temperature of the system.
For endothermic reaction, the value of K increases with increase in temperature and vice versa.
For exothermic reaction, the value of K decreases with increase in temperature and vice versa.