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 Kp.

The equilibrium constant for the given equation is

Explanation:

We are given:

Total pressure in the container = 2.25 atm

The given chemical equation follows:

Initial:              -

At eqllm:         -                   x              2x

Evaluating the value of 'x'

The expression of for above equation follows:

The partial pressure of pure solids and pure liquids are taken as 1 in the equilibrium constant expression.

Putting values in above expression, we get:

Hence, the equilibrium constant for the given equation is

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