{"id":45187,"date":"2019-10-17T17:19:19","date_gmt":"2019-10-17T16:19:19","guid":{"rendered":"https:\/\/www.thermal-engineering.org\/quest-ce-que-la-constante-davogadro-numero-davogadro-definition\/"},"modified":"2019-10-17T17:19:19","modified_gmt":"2019-10-17T16:19:19","slug":"quest-ce-que-la-constante-davogadro-numero-davogadro-definition","status":"publish","type":"post","link":"https:\/\/www.thermal-engineering.org\/fr\/quest-ce-que-la-constante-davogadro-numero-davogadro-definition\/","title":{"rendered":"Qu\u2019est-ce que la constante d\u2019Avogadro – Num\u00e9ro d\u2019Avogadro – D\u00e9finition"},"content":{"rendered":"
\n
6.022 \u00d7 10 ^ 23 a \u00e9t\u00e9 nomm\u00e9 d’apr\u00e8s Avogadro en tant que constante d’Avogadro ou nombre d’Avogadro.\u00a0La constante d’Avogadro est l’une des sept unit\u00e9s de base du SI et est repr\u00e9sent\u00e9e par NA.\u00a0G\u00e9nie thermique<\/span><\/div>\n<\/div>\n
<\/div>\n
\n
\n
<\/div>\n

Nombre d’Avogadro<\/span><\/h2>\n

En hommage \u00e0\u00a0<\/span>Avogadro<\/span><\/strong>\u00a0, le nombre de particules (atomes, mol\u00e9cules, ions ou autres particules) dans\u00a0<\/span>1 mole<\/span><\/strong>\u00a0de substance:<\/span><\/p>\n

6,022 \u00d7 10\u00a0<\/span>23<\/span><\/sup><\/strong><\/p>\n

Il a \u00e9t\u00e9 nomm\u00e9 d’apr\u00e8s Avogadro en tant que\u00a0<\/span>constante d’\u00a0<\/span><\/strong>Avogadro<\/span><\/strong>\u00a0ou\u00a0nombre d’Avogadro<\/strong>\u00a0.\u00a0La constante d’\u00a0Avogadro est l’\u00a0un des sept unit\u00e9s SI de base et repr\u00e9sent\u00e9 par\u00a0<\/span>N\u00a0<\/span><\/em>A<\/span><\/sub>\u00a0.<\/span><\/p>\n

La\u00a0<\/span>loi d’Avogadro<\/span><\/strong><\/a>\u00a0peut \u00eatre utilis\u00e9e pour comparer la m\u00eame substance dans deux conditions diff\u00e9rentes:<\/span><\/p>\n

V\u00a0<\/span><\/em>1<\/span><\/sub><\/em>\u00a0\/ n\u00a0<\/span><\/em>1<\/span><\/sub><\/em>\u00a0= V\u00a0<\/span><\/em>2<\/span><\/sub><\/em>\u00a0\/ n\u00a0<\/span><\/em>2<\/span><\/sub><\/em><\/strong><\/p>\n<\/div>\n<\/div>\n

\n
\n
<\/div>\n

Volume molaire de gaz<\/span><\/h2>\n

L’un des r\u00e9sultats les plus pratiques de cette loi est le\u00a0<\/span>volume molaire d’un gaz<\/span><\/strong>\u00a0,\u00a0<\/span>V\u00a0<\/span>m<\/span><\/sub><\/strong>\u00a0, qui est d’environ:<\/span><\/p>\n

V\u00a0<\/span>m<\/span><\/sub>\u00a0= 22,4 dm\u00a0<\/span>3<\/span><\/sup>\u00a0\/ mol<\/span><\/strong><\/p>\n

Cela signifie que, \u00e0 la temp\u00e9rature standard (273,15 K, 0 \u00b0 C) et \u00e0\u00a0<\/span>la pression atmosph\u00e9rique<\/span><\/a>\u00a0normale\u00a0(101,325 kPa), le volume molaire est le m\u00eame pour tous les gaz id\u00e9aux.\u00a0Notez que c’est dans l’hypoth\u00e8se de gaz parfait.\u00a0Cette valeur d\u00e9pend fortement de la pression et de la temp\u00e9rature.\u00a0Par exemple:<\/span><\/p>\n