Answer: The value of equilibrium constant is 0.997
Step-by-step explanation:
We are given:
Percent degree of dissociation = 39 %
Degree of dissociation,
= 0.39
Concentration of
, c =

The given chemical equation follows:

Initial: c -
At Eqllm:

So, equilibrium concentration of
![N_2O_4=c-c\alpha =[1-(1* 0.39)]=0.61M](https://img.qammunity.org/2021/formulas/chemistry/high-school/dei3psqff3lfdisdpa893ry8ub8qhscrfu.png)
Equilibrium concentration of
![NO_2=2c\alpha =[2* 1* 0.39]=0.78M](https://img.qammunity.org/2021/formulas/chemistry/high-school/kej6zxev7iyjn516xb3jma5po6eag3h2h8.png)
The expression of
for above equation follows:
![K_(c)=([NO_2]^2)/([N_2O_4])](https://img.qammunity.org/2021/formulas/chemistry/high-school/4cen3qjuisdx9zifstby82791mch52oju3.png)
Putting values in above equation, we get:

Hence, the value of equilibrium constant is 0.997