For the decomposition reaction $4 H N O_{3} (g) ⇌ 4 N O_{2} (g) + 2 H_{2} O + O_{2}$ (g) if we start with only the reactant $H N O_{3}$ and p = equilibrium pressure, the equilibrium constant $K_{p}$ is:

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At constant temperature, the equilibrium constant (Kp) for the decomposition reaction. N2O4⇌2NO2 is expressed by, Kp=(4x2P)(1−x2)where, P=pressure, x=extent of decomposition. Which of the following statements is true?

The correct option is D Kp remains constant with change in P and x decreases with pressureKp doesn't change with increase in pressure. However, degree of dissociation, x changes to maintain the equilibrium.

At constant temperature, the equilibrium constant $(K_{p})$ for the decomposition reaction. $N_{2} O_{4} ⇌ 2 N O_{2}$ is expressed by,
$K_{p} = \frac{(4 x^{2} P)}{(1 - x^{2})}$
where, $P =$ pressure, $x =$ extent of decomposition. Which of the following statements is true?

The correct option is D $K_{p}$ remains constant with change in $P$ and $x$ decreases with pressure
$K_{p}$ doesn't change with increase in pressure. However, degree of dissociation, $x$ changes to maintain the equilibrium.