The `N_(2)O_(4)//NO_(2(g))` equilibrium is endothermic as shown below:
`underset(Colourl es)(N_(2)O_(4(g)))hArrunderset(Dark brown)(2NO_(2(g)))`, (`DeltaH=+ve`)
The equilibrium is attained in a container having movable piston by taking `1 mol e` of `N_(2)O_(4(g))` at `50^(@)C` and `1 atm` pressure. At equilibrium, relative molecular mass of the mixture is `65.7`.
If pressure on the mixture is increased, such that volume of mixture becomes half of `I` equilibrium, then:

Options

A. `K_(c)=0.029` and `alpha=0.4`
B. `K_(c)=0.029` and `alpha=0.30`
C. `K_(c)=0.015` and `alpha=0.3`
D. `K_(c)=0.015` and `alpha=0.40`

Explanation

If `V=(37.13)/(2)`, the `K_(c)` remain constant but reaction proceed backward direction.
`:. 0.029=((2alpha_(1))^(2)xx2)/((1-alpha_(1))xx37.13)`
`:. alpha_(1)=0.3`