For gaseous reaction
`aA(g) + bB(g) iff cC(g) + dD(g)`
equilibrium constant `K_c, K_p` and `K_x` are represented by the following relations
`K_c = ([C]^c[D]^d)/([A]^a[B]^b) , K_p = (P"_C^c.P"_D^d)/(P"_A^a.P"_B^b)` and ``K_x = (x"_C^c.x"_C^c)/(x"_A^a.x"_B^b)`
where [A] represents molar concentration of `A, P_A` represents partial pressure of A and P represents total pressure, `x_A`, represents mole fraction of A
On the basis of above work up. Select write option

Options

A. `K_p = K_c(RT)^(Deltan_g), K_x = K_p(RT)^(Deltan_g)`
B. `K_c = K_p(RT)^(-Deltan_g), K_p = K_xP^(Deltan_g)`
C. `K_c = K_xP^(Deltan_g), K_p = K_xP^(Deltan_g)`
D. `K_c = K_p(RT)^(-Deltan_g), K_x = K_p(RT)^(Deltan_g)`

Answer

B