For example:1 mole of atoms = 6.02 ×10 23 atoms1 mole of electrons = 6.02 ×10 23 electrons1 mole of protons = 6.02 ×10 23 protons1 mole of ions = 6.02 ×10 23 ions1 mole of molecules = 6.02 ×10 23 molecules In chemistry, extremely small particles are expressed in moles. Then, the number of atoms present in 12g of carbon-12 is derived as follows:ġ mole = 6.02 ×10 23 particles. The value 6.0 × 1023 is obtained through the following relationship.The mass of one atom of carbon-12 is 1.993 × 10-23 g. It is named after the nineteenth-century Italian chemist, Amedeo Avogadro. The value 6.0 × 1023 is called Avogadro’s constant or Avogadro’s number and is abbreviated as L. That number per mole has been worked by several different experimental methods and is found to be 6.0 × 1023. One mole of each of these different substances contains the same number of the particles (atoms, molecules, ions, electrons, protons, neutrons, etc). The standard unit is called one mole of the substance. A counting unit that is useful in practical chemistry must be used. When carrying out an experiment, a chemist cannot weigh out a single atom, ion, electron, proton or molecule of a substance. The Mole with Other Units of Measurements ![]() THE MOLE CONCEPT AND RELATED CALCULATIONS.
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