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Standard XII

Chemistry

Characteristics of Chemical Equilibrium

According to ...

Question

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

3.11 g/L

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6.22 g/L

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4.56 g/L

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1.56 g/L

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Solution

The correct option is D 3.11 g/L

$N_{2} O_{4}$
$N O_{2}$
Initial moles
1
0
Change
0.2
0.4
Equilibrium moles
$1 - 0.2 = 0.8$
0.4

The molar masses of $N O_{2}$ and $N_{2} O_{4}$ are $46$ g/mol and $92$ g/mol respectively.
The average molar mass of the mixture is $\frac{0.8 \times 92 + 0.4 \times 46}{0.8 + 0.4} = 76.7 g / m o l$
The density of the mixture is $ρ = \frac{P M}{R T} = \frac{1 a t m \times 76.7 g / m o l}{0.0821 L a t m / m o l / K \times 300 K} = 3.11 g / L$

Thus, the correct answer is $A$

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Similar questions

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	$N_{2} O_{4}$	$N O_{2}$
Initial moles	1	0
Change	0.2	0.4
Equilibrium moles	$1 - 0.2 = 0.8$	0.4

According to the reaction gaseous N2O4 dissociates into gaseous NO2N2O4(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 contained in a vessel, then the density of the equilibrium mixture is :