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For the homogeneous gaseous reaction 2 AB2 (g) ⇌ 2 AB (g) + B2 (g) Derive an expression for the degree of dissociation, α, in terms of Kp and total pressure P assuming that α

PCl5 dissociates as: PCl5 ⇌ PCl3 Cl2 If α is the degree of dissociation at certain temperature under atmospheric pressure, then Initial concentration: PCl5 = 1 PCl3 = 0 Cl2 = 0 At Equilibrium: PCl5 = 1 - α PCl3 = α Cl2 = α Total number of moles at equilibrium = 1 – α + ...

Relation between Kp and Kc is given as: Kp = Kc (RT) ∆n Kc = Kp / (RT) ∆n T = 700 K R = 8.314 J mol -1 K-1 ∆n = (2 + 1) – 2 = 1 Kp = 1.8 X 10-3 kPa ...

The Equilibrium constant expression involves the concentrations or partial pressures of the reactants and products. The units of Equilibrium constant K will depend on the number of moles of reactants and products. There are following two cases: Case1. When the total number of moles of products is ...

Effect of addition of inert gas like helium, neon etc has the following effects on the equilibrium constant: There are two cases on which equilibrium depends. These are: (1) Addition of an inert gas at constant volume: When an inert gas is added to the system in equilibrium ...

The reaction will be given as: PCl5 ⇌ PCl3 Cl2 Initial moles: PCl5 = 0.10 PCl3 = 0 Cl2 = 0 Equivalent moles: PCl5 = 0.10 - α PCl3 = α Cl2 = α Total number of moles = 0.10 – α + α + α = 0.10 + α Now, we know that pV = ...

The change of pressure can be observed on the reactions which involves gaseous substances. According to Le-Chateliers’s principle, increase of pressure on a system at equilibrium will shift the equilibrium in the direction in which pressure is reduce. By increase in pressure, the volume occupied by ...

The two French chemists, Le-Chateliers and Braun in 1884 made a certain generalizations to explain the effect of changes of system in equilibrium due to concentration, temperature or pressure. The generalization is known as Le-Chateliers’s principle. When a system is subjected to a change in ...

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