In a closed container for the reaction `A_((g))`+`B_((g))` `harr` `2C_((g))`,`K_(C)=9` .If the initial concentrations of "A,B" and "C" are "1M,1M," and "2M" respectively,then at equilibrium
(1) [A]=[B]=[C]
(2) C=3[A]
(3)"[B],=0.8M
(4) `[A]=[B]!=[C]`

Following equilibrium is established at temperature T. A(g) hArr B(g) + C(g) If equilibrium concentrations of A, B and C are 1M, 2M and 2M respectively, K_​p ​ for the reaction is :-

For a reaction A_((g)) + B_((g))hArrC_((g)) + D_((g)) the intial concentration of A and B are equals but the equilibrium constant of C is twice that of equilibrium concentration of A. Then K is

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

The rate expression for reaction A(g) +B(g) rarr C(g) is rate =k[A]^(1//2)[B]^(2) . What change in rate if initial concentration of A and B increases by factor 4 and 2 respectively ?

The equilibrium constant K_c for the reaction H_2(g)+I_2(g)hArr 2HI(g) is 54.3 at 400^@C . If the initial concentrations of H_2 , I_2 and HI are 0.00623M , 0.00414M , and 0.0224M , respectively, calculate the concentrations of these species at equilibrium.

For the reaction 2A(g)+B(g)hArr C(g)+D(g), K_c=10^(12) .if initially 4,2,6,2 moles of A,B,C,D respectively are taken in a 1 litre vessel, then the equilibrium concentration of A is :