This Law was given by Joseph Proust. According to this law, “A chemical compound always consists of the same elements in the same ratio by weight”. For example, samples of CO2 obtained by different methods always contain the same elements, i.e., carbon and oxygen in the same ratio, i.e., 3: 8 by weight.
This Law was given by Mikhail Lomonosov. This law states that “the total mass can neither be created nor destroyed but can be converted from one form to another during a chemical reaction”. Explanation: Since all the matter is composed of atoms, therefore, atoms can neither be created nor destroyed during a chemical reaction. Total…
The study of relationship between the amounts of reactants and products as indicated by the balanced chemical equation is called stoichiometry. Explanation: Stoichiometry is used to calculate the amount of the product formed or that of the reactant required in a reaction. Stoichiometric calculations are performed by the following assumptions in hand: Reactants are completely…
The volume of one mole of an ideal gas at standard temperature and pressure is called molar volume of a gas and is equal to 22.414 dm3 at STP (Standard temperature & pressure) & 24 dm3 at RTP (Room temperature & pressure). Explanation: At standard temperature and pressure: 2 g of hydrogen (H2) = 1…
The number of atoms, molecules, formula units or ions in one gram atom, one gram molecule, one gram formula unit or one gram ion, respectively is called Avogadro’s number. OR The number of atoms, molecules, formula units or ions in one mole of the substance is called Avogadro’s number. Representation of Avogadro’s Number: It is…
Below are some important points to get clear mole concept, definition of mole chemistry and mole units. Mole can be define as, The atomic mass, molecular mass, ionic mass or formula mass of a substance expressed in grams is called mole of that substance. OR The amount of a substance, which contains 6.02 x 1023…