Exothermic reaction: Exothermic reaction is the reaction where heat energy evolves. C (graphite) + O2 → CO2; ∆H298K = – 393.4 Kj mol-1 Endothermic reaction: Endothermic reaction is the reaction where heat energy absorbed. CaCO3…

Hess’s law is known as after Russian Chemist Germain Hess. Hess helped formulate the early standards of thermochemistry. His famous paper, which was published in 1840, included his law. Hess’s law: If the initial and final condition remains constant the chemical reaction occurs at one…

Ionic product of water: The dissociation of water, H2 O+ ↔ H+ + OH– According to law of mass action, K = [H+] x [OH–] / [H2O] or, K x [H2O] = [H+] x [OH–]…

The conjugated base of strong acid is weak and the conjugated base of weak acid is strong. It can be explain—clearly by reversible reaction. HB ↔ H+ + B– Acid proton base HB is strong…

The principle of Le Chateliar: When a system is at equilibrium, a change in any one of the factors (such as temperature, pressure, concentration) upon which the equilibrium depends will cause the equilibrium to shift…

The constant KC is called the equilibrium constant and applies to reactions in solution. It contains only concentration terms. It should not included terms for (1) any pure solid (ii) any pure liquid, unless it…

Chemical equilibrium: A chemical equilibrium in a system is the state of the system when there is no observable change in the concentration of the reactants and products. Concentration of the reactant and product as…

Dynamic equilibrium: When a reversible reaction reaches at equilibrium, then it seems to be stopped. Because, in this situation there seems to no change in concentration of reactant and products. But in actual the reactions…

In a particular temperature and time the rate of any reaction is proportional to the activation mass (Molar concentration and partial pressure) of the reactants present on that time. Activation mass means, the number of…