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Amedeo Avogadro was born to a respected, wealthy aristocratic family in Northern Italy. He decided not to follow his father's career of law, and instead became a scientist. Avogadro did a lot of great things. A lot of people know his number (the value of which he didn't actually come up with) but today we are going to talk about.

What is Avogadro’s Law?

Avogadro’s Law or Avogadro’s Hypothesis is an Ideal Gas Law that basically defines that how the volume of a gas is directly proportional to the amount of substance (moles) of gas used when pressure and temperature are held constant.

In other words, at constant temperature and pressure, of course, an equal volume of all the gases will have the same number of molecules.

This phenomenon is known as Avogadro’s Principle; named after Italian Chemist, Physicist, and Scientist Amedeo Avogadro who first hypothesized this law in 1811.

In fact, when Avogadro’s Law is substituted with Combined Gas Law (i.e the combination of Boyle’s Law,Charles’s Law, and Gay-Lussac’s Law) develops into an Ideal Gas Law. Moreover, Avogadro’s Law can be deduced from the Kinetic Molecular Theory Of Gas.

Take a look at Top 6 Real-Life Gay Lussac Law Examples

General Consequences and Facts About Avogadro’s Hypothesis

Not to mention, there are some general consequences and easy to remember facts about Avogadro’s Law, which you definitely want to keep in mind:

• If the amount of substance (moles) is increased, the volume will increase. And, vice-versa.
• Like all the other Ideal Gas Law, this Law also describes the behavior of an Ideal Gas. Yet, it can also be applied to real gases at normal temperatures and low pressure.
• In real practice, real gases show a small deviation from the ideal gas behavior. Yet, it is still a useful tool for scientists.
• The molar volume i.e one mole of an ideal gas occupies 22.4 Liters at STP ( i.e at 0°C and 1 atm pressure).
• The Avogadro Number or Avogadro Constant is the number of elementary entities (atoms, molecules, or other particles) present in 1 mole of a substance; represented by NA. Mathematically, it is equal to 6.022×1023.
• This Avogadro Number remains the same for every element; whether the lightest one i.e Hydrogen or the heaviest one i.e Uranium.

Check out, Top 6 Applications of Charles Law

Avogadro’s Law Formula

Amedeo Avogadro Atomic Theory

Recommended, Top 6 Applications of Boyle’s Law

Avogadro’s Law Example Problem

1. A 5 L sample at 27 °C and 3 atm contain 0.600 mol of gas. If we add 0.300 mol of gas at the same pressure and temperature. Then, what will be the final total volume of the gas?

Amedeo Avogadro Law Formula

Avogadro's law is a principle stated by the Italian chemist Amedeo Avogadro (1776-1856) in 1811.

The avagadro's law states that under equal conditions of temperature and pressure, equal volumes of gases contain an equal number of molecules.

Avogadro's number is 6.022 * 10 ²³. This means that 12 grams of carbon-12 contains 6.022 * 10 ²³ carbon-12 atoms.

For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.

The avagadro's law is expressed as: $V\propto n\mathrm{or}\frac{V}{n}=k$
where:
V is the volume of the gas.
n is the amount of substance of the gas (measured in moles).
k is a constant.

Amedeo Avogadro Law Example

Ramus for mac. Because the formula is equal to a constant, Avagadro's law can be rewritten as: $\frac{V1}{n_1}=\frac{V2}{n_2}$

How Was Avogadro's Law Discovered

Example 1:
How many moles are there in one atom?
$\mathrm{No.\; of\; moles}=\frac{1\mathrm{atom}}{6.022x{10}^{23}\mathrm{atoms/mole}}=1.66x{10}^{-24}\mathrm{moles}$