Information about Avogadro's Law
Avogadro's law (Avogadro's Hypothesis, or Avogadro's Principle) is a gas law named after Amedeo Avogadro, who in 1811 hypothesized that:
Thus, the number of molecules in a specific volume of gas is independent of the size or mass of the gas molecules. As an example, equal volumes of molecular hydrogen and nitrogen would contain the same number of molecules, as long as they are at the same temperature and pressure.
The minor aspect of the law can be stated mathematically as:
where:
However, this above equation is just a trivial one, which is valid for all homogeneous substances, including homogeneous liquids and solids. This relation is easy to deduce; its validity was assumed before Avogadro's work.
The most important consequence of Avogadro's law is the following: The ideal gas constant has the same value for all gases. This means that the constant
has the same value for all gases, independent of the size or mass of the gas molecules. This statement is nontrivial, and it embodies Avogadro's ingenious insight into the nature of ideal gases. It took decades to prove Avogadro's law based on the kinetic theory of gases.
One mole of an ideal gas occupies 22.4 liters (dm3) at STP, and occupies 24.45 litres at SATP (Standard Ambient Temperature and Pressure = 25 degrees C and 1 atm/101.3kPa). This volume is often referred to as the molar volume of an ideal gas. Real gases may deviate from this value.
The number of molecules in one mole is called Avogadro's number: approximately 6.022×1023 particles per mole.
Avogadro's law, together with the combined gas law, forms the ideal gas law.
- Equal volumes of gases, at the same temperature and pressure, contain the same number of particles, or molecules.
Thus, the number of molecules in a specific volume of gas is independent of the size or mass of the gas molecules. As an example, equal volumes of molecular hydrogen and nitrogen would contain the same number of molecules, as long as they are at the same temperature and pressure.
The minor aspect of the law can be stated mathematically as:
.
where:
- V is the volume of the gas.
- n is the number of moles in the gas.
- k is a proportionality constant.
However, this above equation is just a trivial one, which is valid for all homogeneous substances, including homogeneous liquids and solids. This relation is easy to deduce; its validity was assumed before Avogadro's work.
The most important consequence of Avogadro's law is the following: The ideal gas constant has the same value for all gases. This means that the constant
- p is the pressure of the gas
- T is the temperature of the gas
has the same value for all gases, independent of the size or mass of the gas molecules. This statement is nontrivial, and it embodies Avogadro's ingenious insight into the nature of ideal gases. It took decades to prove Avogadro's law based on the kinetic theory of gases.
One mole of an ideal gas occupies 22.4 liters (dm3) at STP, and occupies 24.45 litres at SATP (Standard Ambient Temperature and Pressure = 25 degrees C and 1 atm/101.3kPa). This volume is often referred to as the molar volume of an ideal gas. Real gases may deviate from this value.
The number of molecules in one mole is called Avogadro's number: approximately 6.022×1023 particles per mole.
Avogadro's law, together with the combined gas law, forms the ideal gas law.
The gas laws are a set of laws that describe the relationship between thermodynamic temperature (T), pressure (P) and volume (V) of gases. They are a loose collection of rules developed between the late Renaissance and early 19th century.
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Lorenzo Romano Amedeo Carlo Avogadro, Count of Quaregna and Cerreto (August 9, 1776–July 9, 1856) was an Italian savant. He is most noted for his contributions to the theory of molarity and molecular weight.
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18th century - 19th century - 20th century
1780s 1790s 1800s - 1810s - 1820s 1830s 1840s
1808 1809 1810 - 1811 - 1812 1813 1814
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Subjects: Archaeology - Architecture -
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1780s 1790s 1800s - 1810s - 1820s 1830s 1840s
1808 1809 1810 - 1811 - 1812 1813 1814
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Subjects: Archaeology - Architecture -
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molecule is defined as a sufficiently stable electrically neutral group of at least two atoms in a definite arrangement held together by strong chemical bonds.[1][2] In organic chemistry and biochemistry, the term molecule
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The volume of a solid object is the three-dimensional concept of how much space it occupies, often quantified numerically. One-dimensional figures (such as lines) and two-dimensional shapes (such as squares) are assigned zero volume in the three-dimensional space.
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Gas is one of the four major states of matter, consisting of freely moving atoms or molecules without a definite shape. Compared to the solid and liquid states of matter a gas has lower density and a lower viscosity.
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Mass is a fundamental concept in physics, roughly corresponding to the intuitive idea of "how much matter there is in an object". Mass is a central concept of classical mechanics and related subjects, and there are several definitions of mass within the framework of relativistic
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1, −1
(amphoteric oxide)
Electronegativity 2.20 (Pauling scale) More
Atomic radius 25 pm
Atomic radius (calc.) 53 pm
Covalent radius 37 pm
Van der Waals radius 120 pm
Miscellaneous
Thermal conductivity (300 K) 180.
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(amphoteric oxide)
Electronegativity 2.20 (Pauling scale) More
Atomic radius 25 pm
Atomic radius (calc.) 53 pm
Covalent radius 37 pm
Van der Waals radius 120 pm
Miscellaneous
Thermal conductivity (300 K) 180.
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3, 5, 4, 2
(strongly acidic oxide)
Electronegativity 3.04 (Pauling scale)
Ionization energies
(more) 1st: 1402.3 kJmol−1
2nd: 2856 kJmol−1
3rd: 4578.1 kJmol−1
Atomic radius 65 pm
Atomic radius (calc.
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(strongly acidic oxide)
Electronegativity 3.04 (Pauling scale)
Ionization energies
(more) 1st: 1402.3 kJmol−1
2nd: 2856 kJmol−1
3rd: 4578.1 kJmol−1
Atomic radius 65 pm
Atomic radius (calc.
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The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.0221023) entities.
A mole is much like "a dozen" in that both are absolute numbers (having no units) and can describe any type of
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A mole is much like "a dozen" in that both are absolute numbers (having no units) and can describe any type of
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Pressure (symbol: p) is the force per unit area applied on a surface in a direction perpendicular to that surface.
Gauge pressure is the pressure relative to the local atmospheric or ambient pressure.
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Gauge pressure is the pressure relative to the local atmospheric or ambient pressure.
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trillion fold).]]
Temperature is a physical property of a system that underlies the common notions of hot and cold; something that is hotter generally has the greater temperature. Temperature is one of the principal parameters of thermodynamics.
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Temperature is a physical property of a system that underlies the common notions of hot and cold; something that is hotter generally has the greater temperature. Temperature is one of the principal parameters of thermodynamics.
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An ideal gas or perfect gas is a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces. Additionally, the constituent atoms or molecules undergo perfectly elastic collisions with the walls of the container.
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Kinetic theory or kinetic theory of gases attempts to explain macroscopic properties of gases, such as pressure, temperature, or volume, by considering their molecular composition and motion.
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In chemistry and other sciences, STP or standard temperature and pressure is a standard set of conditions for experimental measurements, to enable comparisons to be made between sets of data.
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The molar volume, symbol Vm,[1] is the volume occupied by one mole of a substance (chemical element or chemical compound) at a given temperature and pressure. It is equal to the molar mass (M) divided by the mass density (ρ).
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The Avogadro constant (symbols: L, NA), also called the Avogadro number is the number of "entities" (usually, atoms or molecules) in one mole,[1][2] that is the number of carbon-12 atoms in 12 grams (0.
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The combined gas law is a gas law which combines Charles's law, Boyle's law, and Gay-Lussac's law. These laws each relate one thermodynamic variable to another mathematically while holding everything else constant.
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The ideal gas law is the equation of state of a hypothetical ideal gas, first stated by Benoît Paul Émile Clapeyron in 1834.
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- The state of an amount of gas is determined by its pressure, volume, and temperature according to the equation:
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