[" Problem "7.1],[" The following concentrations were "],[" obtained for the formation of "NH," from "N," ,"],[" and "H_(2)" at equlibrium at "500K" ."],[N_(N),1=1.5times10^(-M),[H_(2)]=3.0times10^(@)M" and "],[" constant."]

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

The following 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 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 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 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 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.