Errors In Avogadro's Law

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