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 is contained in a vessel, then the density of equilibrium mixture is

# Gaseous ${\mathrm{N}}_{2}{\mathrm{O}}_{4}$ dissociates into gaseous ${\mathrm{NO}}_{2}$ according to the reaction ${\mathrm{N}}_{2}{\mathrm{O}}_{4}\left(\mathrm{g}\right)⇌2{\mathrm{NO}}_{2}\left(\mathrm{g}\right)$At 300 K and 1 atm pressure the degree of dissociation of ${\mathrm{N}}_{2}{\mathrm{O}}_{4}$ is 0.2. If one mole of ${\mathrm{N}}_{2}{\mathrm{O}}_{4}$ is contained in a vessel, then the density of equilibrium mixture is

1. A

$1.56\mathrm{g}/\mathrm{L}$

2. B

3. C

4. D

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### Solution:

We have

Total amount of gases, $n={n}_{0}\left(1-\alpha \right)+{n}_{0}\left(2\alpha \right)={n}_{0}\left(1+\alpha \right)=\left(1\mathrm{mol}\right)\left(1+0.2\right)=1.2\mathrm{mol}$

The density of equilibrium mixture is