Any unknown term of this proportion can be found by means of cross-multiplication. Where V is the volume, n is the amount of substance in moles and the subscripts 1 and 2 refer to the initial and final states of a gas in a system. If we consider the pairing of variables at different states (initial and final) of the same process, we can write a proportion: This means the ideal gas constant is the same for all gases. Where k is a constant depending on a given pressure and temperature. Mathematically, the law can be written as The number 6.022 140 76 × 10²³ is called the Avogadro constant.Ī modern statement of Avogadro’s law states:įor a given mass of an ideal gas, its volume and amount in moles are directly proportional if the temperature and pressure maintained constant. One mole of an ideal gas at standard conditions occupies 22.4 liters. For example, one mole of oxygen with an atomic mass of 16 corresponds to 16 grams of this gas. A mole of a substance measured in grams is numerically equal to the average mass of one molecule of the compound, in unified atomic mass units. A mole of a substance is defined as exactly 6.022 140 76 × 10²³ particles (atoms, molecules, ions, or electrons). A balloon filled with helium will be 33 times lighter than a balloon filled with xenon gas.Ī mole is a measure of the quantity of a substance. Note that masses of the different gases will not be the same because they have different molecular masses.
In other words, equal volumes of any gas contain the same number of molecules if the conditions do not change.
Examples of Avogadro’s Law in Real Life SituationsĪerodynamics and Meteorology: Humid Air is Less Dense than Dry AirĪvogadro’s law states that the volume of any gas is proportional to the amount of gas in moles when the temperature and pressure remain constant.
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