Chemical EquilibriumMedium

Question

At 127°C and 1 atm pressure, PCl5(g) is partially dissociated into PCl2(g) and Cl2(g) as PCl5(g) $\rightleftharpoons$PCl3(g) + Cl2(g). The density of the equilibrium mixture is 3.5 g/L. Percentage dissociation of PCl5 is (R = 0.08 L-atm/K-mol,

P = 31, Cl = 35.5)

Options

A.46.28
B.86.16
C.15.86
D.53.72

Solution

$M_{mix} = \frac{dRT}{P} = \frac{3.5 \times 0.08 \times 400}{1} = 112$

Now, $\alpha = \frac{M_{PCl_{5}} - M_{mix}}{(n - 1).M_{mix}} = \frac{208.5 - 112}{(2 - 1) \times 112} = 0.8616$

Create a free account to view solution

View Solution Free
Topic: Chemical Equilibrium·Practice all Chemical Equilibrium questions

More Chemical Equilibrium Questions

CuSO4.5H2O(s) $\rightleftharpoons$CuSO4.3H2O(s) + 2H2O(g), KP for this equilibrium is 1.0 × 10−4 atm2 at 25oC. What is t...The equilibrium of which of the following reactions will not be disturbed by the addition of an inert gas at constant vo...An amount of 4 moles of NH3 gas is introduced with a previously evacuated 1 L container in which it is partially dissoci...Ammonia at a pressure of 10 atm and CO2 at a pressure of 20 atm are introduced into an evacuated chamber. If KP for the ...Consider the following reaction in a sealed vessel at equilibrium with concentrations of $N_{2} = 3.0 \times 10^{- 3}M,O...