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

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.