37.8 g N₂O₅ was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K
$2{\mathrm{N}}_2{\mathrm{O}}_{5\left(\mathrm{g}\right)}\to 2{\mathrm{N}}_2{\mathrm{O}}_{4\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}$
The total pressure at equilibrium was found to be 18.65 bar.
Then, Kp = _______ × 10^–2 [nearest integer]
Assume N₂O₅ to behave ideally under these conditions
Given : R = 0.082 bar L mol^–1 K^–1