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Question

Gaseous N2O4 dissociates into gaseous NO2 according to the reaction N2O4(g)2NO2(g) at 300 K and 1 atm pressure, the degree of dissociation of N2O4 is 0.2. If one mole of N2O4 gas is contained in a vessel, then the density of the equilibrium mixture is :

A
3.11 g/L
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B
4.56 g/L
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C
1.56 g/L
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D
6.22 g/L
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Solution

The correct option is B 3.11 g/L
N2O42NO2

at t=0, moles of N2O4=1, moles of NO2=0

at t=equilibrium, mole of N2O4=1a, mole of NO2=2a

a=degree of dissociation.

Molecular weight of mixture=(1a)×molar mass of N2O4+2a×molar mass of NO2(1a+2a)
=(10.2)(28+64)+2×0.2×(14+32)1+0.2
M=76.66

P=1atm,T=300K,

d=PM/RT

=1×76.660.082×300=3.11 gm/lit .

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