http://www.philosophical-investigations.org/AvogadroRecent Changes of the page "Avogadro" on Philosophical Investigations.en-us http://www.philosophical-investigations.org/Avogadro2009-08-29 04:15:05PerigGouanvic <div id="content" class="wikipage content"> Differences for Avogadro<p><strong></strong></p><table> <tr> <td> <span> Deletions are marked with - . </span> </td> <td> <span> Additions are marked with +. </span> </td> </tr> <tr> <td> Line 2: </td> <td> Line 2: </td> </tr> <tr> <td> <span>-</span> ||||||&lt;tablewidth="60%" bgcolor="#DDDDDD" padding=5px&gt;'''John Dalton''' (1776 - 1844) was able to estimate relative atomic masses of various molecules, the smallest unit that a chemical can exist in without losing its identity. His values were soon improved by '''Amadeo Avogadro''' (1776 - 1856), in 1811. Avogadro made the very important proposal that the volume of a gas (strictly, of an ideal gas ) is proportional to the number of atoms or molecules that are present. Hence, the relative molecular mass of a gas can be calculated from the mass of a sample of known volume.[[br]]BUT neither Avogadro nor Dalton knew how many molecules there were in a given mass of a substance. [[br]]This is historically significant because it means that, although Hahnemann realised that there was a limit to the dilutions that could be used, ''he had no way of knowing what that limit was.''<span>[[FootNote</span>( Source: http://dcscience.net/?p=243 )<span>]]</span>|| </td> <td> <span>+</span> ||||||&lt;tablewidth="60%" bgcolor="#DDDDDD" padding=5px<span>&nbsp;align="left"</span>&gt;'''John Dalton''' (1776 - 1844) was able to estimate relative atomic masses of various molecules, the smallest unit that a chemical can exist in without losing its identity. His values were soon improved by '''Amadeo Avogadro''' (1776 - 1856), in 1811. Avogadro made the very important proposal that the volume of a gas (strictly, of an ideal gas ) is proportional to the number of atoms or molecules that are present. Hence, the relative molecular mass of a gas can be calculated from the mass of a sample of known volume.[[br]]BUT neither Avogadro nor Dalton knew how many molecules there were in a given mass of a substance. [[br]]This is historically significant because it means that, although Hahnemann realised that there was a limit to the dilutions that could be used, ''he had no way of knowing what that limit was.''( Source: http://dcscience.net/?p=243 )|| </td> </tr> </table> </div> http://www.philosophical-investigations.org/Avogadro2009-08-29 04:14:16PerigGouanvic <div id="content" class="wikipage content"> Differences for Avogadro<p><strong></strong></p><table> <tr> <td> <span> Deletions are marked with - . </span> </td> <td> <span> Additions are marked with +. </span> </td> </tr> <tr> <td> Line 1: </td> <td> Line 1: </td> </tr> <tr> <td> </td> <td> <span>+ ||||||&lt;tablewidth="60%" bgcolor="#FFFFE0"&gt; '''Can a homeopathic remedy work if it contains none of the original curative substance?''' ||<br> + ||||||&lt;tablewidth="60%" bgcolor="#DDDDDD" padding=5px&gt;'''John Dalton''' (1776 - 1844) was able to estimate relative atomic masses of various molecules, the smallest unit that a chemical can exist in without losing its identity. His values were soon improved by '''Amadeo Avogadro''' (1776 - 1856), in 1811. Avogadro made the very important proposal that the volume of a gas (strictly, of an ideal gas ) is proportional to the number of atoms or molecules that are present. Hence, the relative molecular mass of a gas can be calculated from the mass of a sample of known volume.[[br]]BUT neither Avogadro nor Dalton knew how many molecules there were in a given mass of a substance. [[br]]This is historically significant because it means that, although Hahnemann realised that there was a limit to the dilutions that could be used, ''he had no way of knowing what that limit was.''[[FootNote( Source: http://dcscience.net/?p=243 )]]||</span> </td> </tr> </table> </div>