neu Table Calculation of Mass of the Name of substance substance taken (gram) Mass of single atom or molecule (gram) Atomic mass or Molar mass/ Avovadro Number No. of atoms or molecules Mass of substance Mass of single atom or molecule 250 S. No. ( 23) (1) 12 6.022 x 100 1.9926 x 10 1 Elemental Carbon (C-12) 1.9926 x 10 INO 6.022 x 10 180 29.89 x 10 2 Glucose (CH 29.89 x 10 1 294.18 3 48.851x10 29418 Potassium dichromate (K, CrO.) -6.022 x 10 48.851 x 10-22 Potassium 158 03 permanganate 158.03 26.242 x 10 6.022 x 10 (KM0 26,242 x 10-22 From the calculations we come to know that 12 g of carbon-12 contains 6.022x104 oms and same numbers of molecules are present in 158.03 g of potassium
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The chemical changes observed in any reaction involve the rearrangement of billions of atoms. It is impractical to try to count or visualize all these atoms, but scientists need some way to refer to the entire quantity. They also need a way to compare these numbers and relate them to the weights of the substances, which they can measure and observe. The solution is the concept of the mole, which is very important in quantitative chemistry.
Avogadro’s Number
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Amedeo Avogadro: Amedeo Avogadro is credited with the idea that the number of entities (usually atoms or molecules) in a substance is proportional to its physical mass.
Amadeo Avogadro first proposed that the volume of a gas at a given pressure and temperature is proportional to the number of atoms or molecules, regardless of the type of gas. Although he did not determine the exact proportion, he is credited for the idea.
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