A sample of pure NO2 is heated to 335 ∘C at which temperature it partially dissociates according to the equation 2NO2(g)⇌2NO(g)+O2(g) At equilibrium the density of the gas mixture is 0.525 g/L at 0.750 atm .

The equilibrium constant for the reaction is 0.00662

Explanation:

The balanced chemical equation is :

2NO2(g)⇌2NO(g)+O2(g

At t=t  1-2x ⇔ 2x + x moles

The ideal gas law equation will be used here

PV=nRT

here n= = = density

P =       density is 0.525g/L, temperature= 608.15 K, P = 0.750 atm

putting the values in reaction

0.75 =

  M    = 34.61

to calculate the Kc

Kc=

  x M NO2 + M NO+ M O2

Putting the values as molecular weight of NO2, NO,O2

34.61=

x= 0.33

Kc=

    putting the values in the above equation

Kc = 0.00662

it is b that is the answer.