For following equilibrium: N2O4( g)2NO2( g)   ; KP=PNO22PN2O4; Graph between Ptotal Vs α is given. Where Ptotal = Total pressure at equilibrium a ® degree of dissociation (a << 1) 

 

  1. A

    value of KP is 36 atm. 

  2. B

    value of P2 is 56.25 atm. 

  3. C

    If total pressure is increased at equilibrium then reaction will move in backward direction. 

  4. D

    On increasing temperature degree of dissociation of N2O4 (g) will increase.

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    Solution:

     

    N2O4( g)a  0-a0α    2 NO2(g  )   2a0α             KP=4α21-α2·Pt4α2·Pt  if α<<1

    (1) KP=4×(0.3)2×100=36 atm  KP=4α22P2 4×(0.3)2×100=4(0.4)2P2

    (2) P2=90016=56.25 atm

    (3) QP=4α2. Pt so if Pt increases then α decreases to reset QP=KP.

    (4) As reaction is endothermic in forward direction so on increasing temperature, it favour endothermic step i.e. α increases. 

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