Two equilibrium reactions of nitrogen with oxygen, with their corresponding equilibrium constants (Kc) at a certain temperature, are given below. reaction (1): N2(g) + O2(g) 2 NO(g); Kc = 1.54e-31 reaction (2): N2(g) + 1/2 O2(g) N2O(g); Kc = 2.61e-24 Using this set of data, determine the equilibrium constant for the following reaction, at the same temperature. reaction (3): N2O(g) + 1/2 O2(g) 2 NO(g)

Kc = 1.54e - 31 / 2.61e - 24

Explanation:

1 )    ; Kc = 1.54e - 31

2)    ; Kc = 2.16e - 24

   upon reversing  ( 2 )  equation

        Kc = 1/2.16e - 24  

    now adding 1 and reversed equation (2)

   we get ,

                   Kc = 1.54e-31 × 1/2.61e - 24

       equilibrium constant of equation (3) is -

            Kc = 1.54e - 31 / 2.61e - 24

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