Deviation from Ideal Gas Law Practice Test

The real pressure is higher because strong attractions at high pressure pull molecules away from the walls, decreasing collisions and increasing pressure.

The real pressure is higher because the ideal gas law assumes particles have volume, so it underestimates pressure at high pressure.

The real pressure is higher because $PV=nRT$ only applies when temperature is changing, not when pressure is high.

The real pressure is higher because at high pressure the finite volume of gas particles reduces free space, increasing collision frequency with the walls.

The real pressure is higher because NH$_3$ decomposes into N$_2$ and H$_2$ at high pressure, increasing $n$ and raising pressure.