Answer to Question #209498 in Physical Chemistry for Khamis

Question

  A flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 oC and allowed to reach equilibrium. When equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) What are the partial pressures of NO2 and N2O4 at equilibrium? 

  (b) Calculate Kp and Kc for following reaction at 25 oC. 

      2 NO2(g) ⇄ N2O4(g)

Answer 1

a) 1.762atm

b)$K_c=68.5Lmol^{-1}$