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= [tex]\frac{w}{W}[/tex] = [tex]\frac{w}{V}[/tex]= density
P = [tex]\frac{density RT}{M}[/tex] density is 0.525g/L, temperature= 608.15 K, P = 0.750 atm
putting the values in reaction
0.75 = [tex]\frac{0.525 x 0.0821 x 608.15 }{M}[/tex]
M = 34.61
to calculate the Kc
Kc=[tex]\frac{ [NO] [O2]}{NO2}[/tex]
[tex]\frac{1-2x}{1+x}[/tex] x M NO2 + [tex]\frac{2x}{1+x}[/tex] M NO+ [tex]\frac{x}{1+x}[/tex] M O2
Putting the values as molecular weight of NO2, NO,O2
[tex]\frac{46(1-2x) +30(2x)+32x}{1+x}[/tex]
34.61= [tex]\frac{46}{1+x}[/tex]
x= 0.33
Kc= [tex]\frac{4x^2)x}{1-2x^2}[/tex]
putting the values in the above equation
Kc = 0.00662
