There are two types of chemical equilibria: 1. Homogeneous equilibrium 2. Heterogeneous equilibrium 1. Homogeneous equilibrium: The equilibrium reactions in which all the reactants and the products are in the…
Applications of the equilibrium constant 1. The magnitude of the equilibrium constant : The magnitude of the equilibrium constant K means the extent to which a reaction can proceed i.e.…
The important characteristics of equilibrium constant are discussed below: 1. The equilibrium constant has a definite value for every reaction at a particular temperature. 2. The value of equilibrium constant…
Reaction will be given as: H2 (g) + I2 (g) = 2 HI (g) Therefore, the equilibrium constant K will be given as: K = 2 / The molar concentrations…
The given equation is: 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) Therefore the equilibrium constant Kc, will be given as: Kc = 2 / 2 Initial molar…
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…
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…
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 =…
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…
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…
admin