The given equation is: 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) Therefore the equilibrium constant Kc, will be given as: Kc = [N2O] 2 / [N2] 2 [O2] Initial molar concentrations are: [N2] = 0.482 mol / 10.0 L = 0.0482 mol L-1 [O2] = 0.933 mol ...

Reaction will be given as: H2 (g) + I2 (g) = 2 HI (g) Therefore, the equilibrium constant K will be given as: K = [HI] 2 / [H2] [I2] The molar concentrations of the species at equilibrium are: [H2] = 0.4 / 5 = 0.08 mol L-1 [I2] = 0.4 ...

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 is independent of the original concentration of reactants. 3. The value of equilibrium constant tells the extent to which a reaction ...

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. measuring the completion of the reversible reaction. If the value of K is larger, then the equilibrium concentration ...

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 same phase are known as homogeneous equilibrium reactions. These are divided into two categories: (a) The number of product molecules is equal ...

Stoichiometric coefficient: The number of molecules of a reactant taking part in a reaction is known as Stoichiometric coefficient. For example: Consider the following equation: aA + bB ⇌ cC + dD In this equation, a, b, c and d are called as Stoichiometric coefficients of the A, B, ...

Relationship between Kp and Kc Consider the following reversible reaction: aA + bB ⇌ cC + dD The equilibrium constant for the reaction expressed in terms of the concentration (mol / litre) may be expressed as: K c = [C] c [D] d / [A] a [B] b If the ...

Norwegian Chemists Waage and Gulberg were the ones who gave us law of mass action. This law of mass action suggest a quantitative relationship between the rates of the reaction and the concentration of the reacting substances. Law of mass action states that: The rate of a ...