At equilibrium, the concentration of `A_(2)`(g), `B_(2)`(g) and AB(g) are `1times10^(-2)`M, `2times10^(-2)`M" and `4times10^(-2)`M respectively in a sealed vessel at "273K" .The value of `K_(C)` for the reaction `A_(2)`(g)+ `B_(2)`(g) `harr` 2AB(g) is
A )4
B) 16
C) 6
D) 8

The factor which changes equilibrium constant of the reaction A_(2)(g)+B_(2)(g) rarr 2AB(g) is

The relation between K_(P) and K_(C) for the reaction A(g)+B(g) hArr C(g)+2D(g) is -

At 800 K in a sealed vessel for the equilibrium N_(2)(g) + O_(2) (g) hArr 2NO(g), the equilibrium concentrations of N_(2) (g), O_(2)(g) and NO(g) are respectively 0.36xx10^(-3) M, 4.41 xx 10^(-3) M and 1.4 xx 10^(-3) M. Calculate the value of K_(c) for the reaction NO(g) hArr 1//2 N_(2)(g) +1//2 O_(2) (g) at 800 K is :

The K_c for given reaction will be A_2 (g) +2B (g) hArr C(g) +2D(s)

For the reaction equilibrium, N_(2)O_(4(g))hArr2NO_(2(g)) , the concentration of N_(2)O_(4) and NO_(2) at equilibrium are 4.8xx10^(-2) and 1.2xx10^(-2) mol/L respectively. The value of K_(c) for the reaction is:

At equilibrium, the concentrations of N_(2)=3.0xx10^(-3)M, O_(2)=4.2xx10^(-3) M, and NO=2.8xx10^(-3) M in a sealed vessel at 800K . What will be K_(c) for the reaction N_(2)(g)+O_(2)(g)N_(2)(g)+O_(2)(g)hArr2NO(g)2NO(g)

For an equilibrium reaction, N_(2)O_(4)(g) hArr 2NO_(2)(g) , the concentrations of N_(2)O_(4) and NO_(2) at equilibrium are 4.8 xx 10^(-2) and 1.2 xx 10^(-2) mol//L respectively. The value of K_(c) for the reaction is

For the reaction equilibrium , N_2O_4(g) hArr 2NO_(2)(g) the concentrations of N_2O_4 and NO_2 at equilibrium are 4.8xx10^(-2) and 1.2xx10^(-2) mol L^(-1) respectively.The value of K_C for the reaction is :