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Question

For the equilibrium at 298 K; N2O4(g)2NO2(g);GN2O4=100kJmol1 and GNO2=50kJmol1. If 5 mol of N2O4 and 2 moles of NO2 are taken initially in one litre container than which statement are correct

A
reaction proceeds in forward direction
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B
Kc=1
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C
ΔG=0.55kJ,ΔG=0
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D
At equilibrium [N2O4]=4.84M and [NO2]=0.212M
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Solution

The correct options are
A reaction proceeds in forward direction
B Kc=1
C ΔG=0.55kJ,ΔG=0
ΔG=ΔG+2.303RTlogQ

ΔG=2×GNO2GN2O4=2×50100=0

ΔG=0+2.303×8.314×103×298log225=00.55kJ

ΔG=0.55kJ, i.e, reaction proceeds in forward direction

Also ΔG=0=2.303RTlogKK=1

Now, N2O455x=2NO222+2x

Kp=(PNO2)(PN2O4)=1=(2+2x)25x or x=0.106

So, [N2O4]=5x=4.894M, [NO2]=2+2x=2.12M

Hence, options A, B and C are correct.

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