Chemical EquilibriumHard
Question
In an evacuated vessel of capacity 112 L, 4 moles of Ar(g) and 5 moles of PCl5(g) were introduced and the temperature is maintained at 273oC. At equilibrium, the total pressure of the mixture was found to be 4.8 atm.
Options
A.The degree of dissociation of PCl5(g) into PCl3(g) and Cl2(g) is 0.6.
B.KP for the reaction: PCl5(g) $\rightleftharpoons$PCl3(g) + Cl2(g) is 2.7 atm.
C.At equilibrium, the total moles of gases are 12.
D.On removing Ar(g) from the equilibrium mixture at constant pressure and temperature, the extent of dissociation of PCl5 will increase.
Solution
PCl5(g) $\rightleftharpoons$PCl3(g) + Cl2(g)
Initial moles 5 0 0
Moles at equilibrium 5 – x x x
From question, $(5 - x) + x + x + 4 = \frac{4.8 \times 112}{0.0821 \times 546} \Rightarrow x = 3$.
$\therefore\alpha = \frac{x}{5} = 0.6\text{ and }K_{P} = \frac{x.x}{5 - x}.\left( \frac{4.8}{12} \right) = 1.8\text{ atm}$
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