LAWS OF CHEMICAL COMBINATIONS
Topics to be covered during this article
- Law of Conservation of Mass
- Law of Definite Proportions
- Law of Multiple Proportions
- Gay Lussac’s Law of Gaseous Volumes
- Avogadro Law
- Dalton's Atomic Theory
- Atoms and Molecules
- Atomic Mass Unit
- Gram mass
- Molecular Mass
- Gram Molecular Mass
- Formula Mass
- Mole Concept
- Molar Volume
- Conclusion
Law of Conservation of Mass
(Given by Lavoisier in 1789).It states that matter (mass) can neither be created nor destroyed.
Law of Fixed Proportions or Constant Composition
This law was proposed by Louis Proust in 1799, which states that: 'A compound always consists of an equivalent elements combined together within the same ratio, regardless of the tactic of preparation or the source from where it's taken'.
Law of Multiple Proportions
This law is Proposed by Dalton in 1803, this law states that: 'When two elements combine to make two or more compounds, then the various masses of 1 element, which combine with a hard and fast mass of the opposite , bear an easy ratio to at least one another'.
Gay Lussac’s Law of Gaseous Volumes
(Given by Gay Lussac in 1808.) According to the present law when gases combine or are produced during a reaction they are doing so during a general ratio by volume arranged all gases are at equal temperature and pressure.
e.g.H2(g) + Cl2(g) →2HCl(g)
All reactants and products have an easy ratio 1:1:2.
Avogadro Law
(In 1811, Given by Avogadro) consistent with this law equal volumes of gases at an equivalent temperature and pressure should contain an equal number of molecules.
Dalton's Atomic Theory
*All substances are made from tiny, indivisible particles called atoms.
*Atoms of an equivalent element are identical in shape, size, mass and other properties.
*Atoms of various elements are different altogether respects.
*Atoms are the littlest unit that takes part in chemical reactions.
*Atoms combine with one another in simple integer ratios to make molecules.
*Atoms can't be created, divided or destroyed during any chemical or phase change .
Atoms and Molecules
Atomic Mass Unit
One mass unit is defined as a mass exactly adequate to one twelfth the mass of 1 carbon -12 atom. And 1 amu = 1.66056×10–24 g. Today, ‗amu‘ has been replaced by ‗u‘ which is understood as unified mass. mass mass of a component is defined because the average relative mass of an atom of a component as compared to the mass of an atom of carbon -12 taken as 12.
Gram mass
The quantity of a component whose mass in grams is numerically adequate to its mass . In simple terms, the mass of a component expressed in grams is that the gram mass or gram-atomic weight .
For example, the mass of oxygen = 16 amu Therefore gram mass of oxygen = 16 g
Molecular Mass
Molecular mass of a substance is defined because the average relative mass of its molecule as compared to the mass of an atom of C-12 taken as 12. It expresses on what percentage times the molecule of a substance is heavier than 1/12th of the mass of an atom of carbon.
For example, a molecule of CO2 is 44 times heavier than 1/12th of the mass of an atom of carbon. So, the molecular mass of carbon di oxide is 44 amu. it's obtained by adding the atomic masses of all the atoms present in one molecule.
Gram Molecular Mass
A quantity of substance whose mass in grams is numerically adequate to its molecular mass is named gram molecular mass. In simple terms, the molecular mass of a substance expressed in grams is named gram molecular mass.
e.g., the molecular mass of oxygen = 32 amu Therefore, gram molecular mass of oxygen = 32 g
Formula Mass
Sum of atomic masses of the weather present in one formula unit of a compound. it's used for the ionic compounds.
Mole Concept
Mole is defined because the amount of a substance, which contains an equivalent number of chemical units (atoms, molecules, ions or electrons) as there are atoms in just 12 grams of pure carbon-12. A mole represents a set of 6.022 x1023( Avogadro's number) chemical units. The mass of 1 mole of a material in grams is called its molar mass.
Molar Volume
The volume occupied by one mole of any substance is named its molar volume. it's denoted by Vm. One mole of all gaseous substances at 273 K and 1 atm pressure occupies a volume adequate to 22.4 litre or 22,400 mL. The unit of this volume is litre per mol or millilitre per mol.
Conclusion
In this article, we've learned many laws and Dalton's Atomic Theory and also all terms which are associated with atoms and molecules. I hope you wish this article. Share this article to your friends. And Please send your feedback through comments.