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  4. The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction PCl5(g) arrow PCl3(g)+Cl2(.g.) . Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)

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Q. The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction

$PCl_{5}\left(g\right) \rightarrow PCl_{3}\left(g\right)+Cl_{2}\left(\right.g\left.\right)$ . Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)

NTA AbhyasNTA Abhyas 2020Equilibrium

Solution:

$\begin{array}{cccc} & PCl _{5}( g ) & \rightleftharpoons PCl _{3}( g )+ Cl _{2}( g ) \\ t =0 & a & 0 & 0 \\ t _{ eq } & 0.6 a & 0.4 a & 0.4 a \end{array}$

$n_{Total}=1.4a$

$\therefore \, \, M_{a v}=\frac{208 \, a}{1.4 \, a} \\ \\ \, =148.57 \\ \\ \therefore \, \, P_{m i x}=\frac{P_{M_{a v}}}{R T} \\ \\ \, \, =\frac{1 \times 148.57}{0.0821 \times 420}=4.30$