Question

A sample of solid NH₄NO₃ is placed in an empty container. It decomposes according to the following reaction:

         NH₄NO₃(s) $LaTeX: \Leftrightarrow$ ⇔ N₂O(g) + 2H₂O(g)

At equilibrium, the total pressure in the container is 2.25 atm. Calculate K_p.

Answer 1

. Given reaction NHL NO₂ N₂O + 2H₂O First we will develop the ICE table to find the equilibrium pressure constant (xp) NH y No No 2H₂O - C5) (og Initial breasure o O o o tn tan Equilibrium pressure Change an Next, the total equilibrium pressure is equal to the partial pressure of individual gases (Here WHY NO is not considered because it is solid) Ptoral = PA +Pa So, here - Ptotal = NO2 H₂O Ptotal = a tan = 3n Given total = 2.25 atm . 2.25 = 3n no 2.25/3 or = 0.75

kp is the equilibrium constant pressure calculated from the partial pressure of a reachon equation. - Kp = [N2o] [H₂07² or, kp = [n] [an]? = 423 We calculated the value of n = 0.75. Substituting the value of n, we get kp So Kp = 4 (0.753 - lag Crounded to 2 decimal places) Answer Kp = 1.69 - Answer.