Mass cannot be created nor destroyed in a chemical reaction
Explanation:
The law of conservation of mass was stated by Antoine lavoisier in 18th century which states that for a isolated system the mass can neither be created nor be destroyed in a chemical reaction. It means that the total mass of the reactants is equal to the total mass of the product formed i.e there is no change in the mass of the reactants even after the reaction which is stated by the law of the conservation of the mass.
The mass of the elements are not created or destroyed but their form is changed to another form of atoms or molecules with conserved mass.
For a balanced chemical equation of the formation of the water, 4 grams of hydrogen combines with 32 grams of the oxygen to give 36 grams of the water where the sum of the mass of the reactant is equals to the mass of the product.
The law is given by the following equation: PV = nRT, where P = pressure, V = volume, n = number of moles, R is the universal gas constant, which equals 0.0821 L-atm / mole-K, and T is the temperature in Kelvin.
