The following concentrations were obtained for the formation of `NH_(3)` from `N_(2)` and `H_(2)` at equilibrium at `500 K`. `[N_(2)]=1.5xx10^(-2) M, [H_(2)]=3.0xx10^(-2)M,` and `[NH_(3)]=1.2xx10^(-2)M`. Calculate the equilibrium constant.

The following concentrations were obtained for the formation of NH_(3) from N_(2) and H_(2) at equilibrium at 500K . [N_(2)]=1.5xx10^(-2)M . [H_(2)]=3.0xx10^(-2) M and [NH_(3)]=1.2xx10^(-2)M . Calculate equilibrium constant.

The following concentration were obtained for the formation of NH_(3)(g) from N_(2)(g) and H_(2)(g) at equilibrium and at 500 K: [N_(2)] = 1 xx 10^(-2)M, [H_(2)] = 2 xx 10^(-2)M and [NH_(3)] = 2xx 10^(-2)M . The equilibrium constant, K_(c) , for the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) at 500 K is

The following concentrations were obtained for the formation of NH_3 from N_2 and H_2 at equilibrium at 500K. [N_2] = 1.5 xx 10^-2M. [H_2] = 3.0 xx10^-2 M and [NH_3] =1.2 xx 10^-2 M . Calculate equilibrium constant.

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))hArr2NH_(3(g)) [N_(2)]=1.5xx10^(-2)M,[H_(2)]=3.0xx10^(-2)M,[NH_(3)]=1.2xx10^(-2)M Calculate the equilibrium constant.

The following concentration were obtained for the formation of NH_3 from N_2 and H_2 at quilibrium at 500 k. It (N_2(g)=1.5xx10^-2M,(H_2(g)=3.0xx10^-2M and (NH_3(g)=1.2xx10^-2M .Calculate equilbrium constant

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.