For the reaction `A(g) iff B (g), K_(C)=10`
`B(g) iff C(g), K_(C)=2`
`C(g) iff D(g), K_(C)=0.01`
Calculate `K_(C)` for the reaction `D(g) iff A(g)`.

Calculate K_(P) for the reaction A(g) iff B(s)+2C(g), K_(C)=0.2 at 305 K.

Calculate K_(P) for the reaction A(g) iff B(s)+2C(g), K_(C)=0.2 at 305 K.

Calculate K_(P) for the reaction A(g) iff B(s)+2C(g), K_(C)=0.2 at 305 K.

For the reaction (1) and (2) A(g) iff B(g)+C(g) .....(1) X(g) iff 2Y(g) ....(2) Given, K_(p_1):K_(p_2) = 9:1 If the degree of dissociation of A(g) and X(g) be same then the total pressure at equilibrium (1) and (2) are in the ratio :

For the reaction 2NO_(2)(g) iff 2NO(g)+O_(2)(g), K_(c)=4 times 10^(-6) at 500 K. Hence, the K_(c) of the reaction NO(g)+1/2O_(2)(g) iff NO_(2)(g) at 500 K is

K_1 and K_2 are the respective equilibrium constants for the following two reactions : (i) N_2 (g) + O_2 (g) iff 2NO(g) (ii) 2NO(g) + O_2(g) iff 2NO_2(g) Then the equilibrium constant for the reaction N_2 (g) + 2O_2(g) iff 2NO_2(g) will be

For the reaction, 2NH_3(g) iff N_2(g) + 3H_2(g) the units of K_p will be