• Avogadro's Law States That
• Avogadro's Law States That Quizlet
• Avogadro's Law States That
• Avogadro's Law States That For An Ideal Gas

Avogadro's law states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. More exactly, it also includes single atoms, e.g. For a case of noble gases, due the way how IUPAC defines a molecule. Avogadro’s law also called Avogadro’s principle or Avogadro’s hypothesis, is a gas law that states the entire variety of atoms or molecules of a gas (i.e., the quantity of volatilised substance) is directly proportional to the amount occupied by the gas at constant temperature and pressure.

Avogadro's Law and the Ideal Gas Law

Avogadro's Law is the relation which states that at the same temperature and pressure, equal volumes of all gases contain the same number of molecules. The law was described by Italian chemist and physicist Amedeo Avogadro in 1811. Avogadro’s Law states that: 1 mole of every gas occupies the same volume, at the same temperature and pressure. At STP (standard temperature and pressure), this volume is 22.4 liters At RTP (room temperature and pressure), this volume is 24 dm 3 (liters) We can also say: The molar volume of a gas is 22.4 liters at STP (standard temperature. Because R is a constant, we can use the qualities of any gas — its temperature, pressure, volume, and number of moles — to determine the value of R. Avogadro’s law states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.

Molecular Meanings

The volume of one mole of any gas at standard temperature and pressure is called the molar volume.

It may not seem immediately obvious why all gases should have the same molar volumes at the same temperatures. Consider this: If the pressure of a gas is equal to the force exerted by gas particles pushing on the sides of whatever container it's stored in, and the volume of a gas depends on its pressure (Boyle's Law), then the molar volumes of every gas are the same. This principle was first understood by Amadeo Avogadro, and is usually referred to as Avogadro's Law.

You've Got Problems

Problem 4: If my oven has a volume of 1,100 L, a temperature of 250 C, and a pressure of 1.0 atm, how many moles of gas does it hold?

Let's see an example of how this works:

Chemistrivia

Avogadro's Law States That

The ideal gas law explains why hot air balloons work. The number of moles of air inside the balloon will be less than the number of moles of air outside the balloon because the air inside the balloon is warmer than the outside air. Because there are fewer moles of air inside the balloon than outside, the mass of the air in the balloon is also less, causing the balloon to 'float' above the surrounding cold air.

Avogadro's Law States That Quizlet

Excerpted from The Complete Idiot's Guide to Chemistry 2003 by Ian Guch. All rights reserved including the right of reproduction in whole or in part in any form. Used by arrangement with Alpha Books, a member of Penguin Group (USA) Inc.

Avogadro's Law States That

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Avogadro's Law States That For An Ideal Gas

The lab calculations resulted in an average of 21.7L/mol which was fairly close to the theoretical value, 22.4L/mol. In order to obtain that result through calculations, the water vapor pressure and the water height correction had to take place. After, the combined gas law had to be utilized and manipulated to find the volume and divide that volume by moles of magnesium. Being close to the theoretical value, 22.4L, it verifies that one mole of all gases occupy 22.4L in any container under standard temperature and pressure. This information could be valuable in many ways. For example, it proves Avogadro’s Law which states that at a standard temperature and pressure, one mole of any gas will occupy the same value which is 22.4L. Like a puzzle piece, once discovered, it…show more content…
For instance, Avogadro’s Law helped introduce the ideal gas law theory which stated how pressure, volume, temperature, and moles interact with each other.
While conducting the experiment, there were multiple opportunities for errors to arise. One of the most drastic errors were the air bubbles stuck inside the eudiometer. The air bubbles contained hydrogen gas and were stuck on the sides instead of rising up into the collection of gas. This would have shifted the volume of the hydrogen gas higher than the actual value and ultimately increase the molar volume of the gas. Another example of an error is the measuring of the ribbon of magnesium. The ribbon of magnesium was not straightened out all the way, and this resulted in a length which is lower than the real value. When converting length into mass and into moles, there would be a significant margin of error. The error would shift the molar volume much lower than it is. Another way the measuring of magnesium could have resulted in the error was