Question

When solid ammonium carbamate sublimes, it dissociates completely into ammonia and carbon dioxide according to the following equation: At 50 °C, experiment shows that the total pressure of the gases in equilibrium with the solid is 0.596 atm. What is the equilibrium constant, ?

Answer 1

Answer: The equilibrium constant for the given equation is 0.0315

Step-by-step explanation:

We are given:

Total pressure in the container = 0.596 atm

The given chemical equation follows:

`N_2H_6CO_2(s)\rightleftharpoons 2NH_3(g)+CO_2(g)`

Initial: -

At eqllm: - 2x x

Evaluating the value of 'x'

`\Rightarrow (x+2x)=0.596\\\\x=0.199`

The expression of
`K_p` for above equation follows:

`K_p=p_(CO_2)* (p_(NH_3))^2`

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:

`K_p=(0.199)* (2* 0.199)^2\\\\K_p=0.0315`

Hence, the equilibrium constant for the given equation is 0.0315