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

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:

$K_p=p_{CO_2}\times (p_{NH_3})^2$

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:

$K_p=(0.199)\times (2\times 0.199)^2\\\\K_p=0.0315$

Hence, the equilibrium constant for the given equation is 0.0315