Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2. N2O4 (g) ⇌ 2 NO2 (g) (a) The equilibrium constant Kc at 25°C is 0,125. What percentage of dinitrogen tetroxide is dissociated when 0,0300 mol N2O4 is placed in a 1,00 dm3 flask and left to reach equilibrium? (b) The amount of nitrogen dioxide formed increases as the temperature rises. Is the dissociation of N2O4 endothermic or exothermic?

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Q: The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698 K: 2HI(g)  H2(g) +…

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