Given the following reaction: N2O4(g) yields 2NO2(g). If only 37%of N2O4(g) dissociated, what is the value of the equilibrium constant? Given: [N2O4] = 1.0M

Kc = 0.22

Explanation:

          N₂O₄(g)       =>    2NO₂(g)

C(i)      100%                      0%

ΔC       -37%                  +37%

C(eq)   100% - 37%         37%

           = 63%

Kc = [NO₂]²/[N₂O₄] = (37%)²/(63%) = (37/100)²/(63/100) = (0.37)²/(0.63) = 0.22

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