The equilibrium between NO2 and N2O4 can be described by the following equation:

2NO2(g) ⇌ N2O4(g) Kp = 7.0

If a sealed flask contains 1.5 atm of NO2 and 14.2 atm of N2O4. Calculate the value of Kc for the reaction,

The question is incomplete, here is the complete question:

The equilibrium between NO₂ and N₂O₄ can be described by the following equation:

2NO₂(g) ⇌ N₂O₄(g); Kp = 7.0

If a sealed flask contains 1.5 atm of NO₂ and 14.2 atm of N₂O₄. Calculate the value of Kc for the reaction at 25°C

The value of for given reaction is 171.3

Explanation:

For the given chemical equation:

Relation of is given by the formula:

Where,

= equilibrium constant in terms of partial pressure = 7.0

= equilibrium constant in terms of concentration

R = Gas constant =

T = temperature =

= change in number of moles of gas particles =

Putting values in above equation, we get:

Hence, the value of for given reaction is 171.3