The equilibrium constant at 850 ~K for the reaction N ₂(g)+ O ₂(g) 2 NO (g) is 0.5625 . The equilibrium concentration of NO (g) is 3.0 10⁻³ M . If the equilibrium concentrations of N ₂(g) and O ₂(g) are equal, the concentrations of N ₂(g) in M is

Step-by-step solution

Given, N ₂(g)+ O ₂(g) 2 NO (g) i.e. equilibrium constant, K_C=0.5625 Equilibrium concentration of [ NO ]=3 10⁻³ M array rlrl & & K_C & = [ NO ^2 . [ N ₂ ] [ O ₂ ] & But, & [ N ₂ ] & = [ O ₂ ] (Given) & & K_C & = [ NO ]^2 [ ~N ₂ ]^2 & & & or, & 0.5625 & = [3 10⁻³ ]^2 [ ~N ₂ ]^2 & or, & [ N ₂ ]^2 & = [3 10⁻³ ]^2 0.5625 = 9 10⁻⁶ 0.5625 & or, & [ N ₂ ]^2 & =16 10⁻⁶ or, & [ N ₂ ] & =4 10⁻³ array Hence, option (a) is the correct answer.