Calculate the equilibrium constant (K) for the formation of NH^ in the following reaction: `N_2(g) + 3H_2(g) At equilibrium, the concentration of `NH_3`, `H_2` and `N_2` are `1.2 xx 10^(-2) ,3.0 xx 10^(-2)` and `1.5 xx 10^(-2)` M respectively.

Calculate the equilibrium constant (Kc) for the formation of NH_(3) in the following reactions. N_(2)(g) +3H_(2)(g) hArr 2NH_(3)(g) At equilibrium, the concentration of NH_(3), H_(2) and N_(2) are 1.2 xx 10^(-2), 3.0xx10^(-2) and 1.5xx10^(-2) respectivley.

Write the equilibrium constant expression for the following equilibria: N_2(g) +3H_2hArr 2NH_3(g)

For the equilibrium system 2HX(g) hArr H_(2)(g)+X_(2)(g) the equilibrium constant is 1.0xx10^(-5) . What is the concentration of HX if the equilibrium concentration of H_(2) and X_(2) are 1.2xx10^(-3) M, and 1.2xx10^(-4) M respectively?

Unit of equilibrium constant (K_c) for the reaction N_2(g)+3H_2(g)

What is concentration quotient ? Write concentration quotients for the the following reactions: N_2(g) + 3H_2(g) hArr 2NH_3(g)

The equilibrium constant for the reaction H_(2)(g)+I_(2)(g)hArr 2HI(g) is 32 at a given temperature. The equilibrium concentration of I_(2) and HI are 0.5xx10^(-3) and 8xx10^(-3)M respectively. The equilibrium concentration of H_(2) is

The equilibrium constants for A_2 (g) hArr 2A(g) at 400 k and 600 k are 1xx 10^(-8) and 1 xx 10^(-2) respectively . The reaction is

The following concentration were obtained for the formation of NH_3 from N_2 and H_2 at equilibrium for the reaction N_2(g) +3H_2(g) hArr 2NH_3(g) [N_2]=1.5 xx 10^(-2) M [H_2]=3.0 xx 10^(-2) M [NH_3]=1.2 xx 10^(-2) M Calculate equilibrium constant.

The equilibrium constant for the reaction N_2+3H_2 hArr 2NH_3 is K , then the equilibrium constant for the equilibrium 2NH_3hArr N_2+3H_2 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 4.8 xx 10^(-2) and 1.2 xx 10 ^(-2) " mol " L^(-1) respectively . The value of K_c for the reaction is