{"id":1177,"date":"2015-10-23T06:02:11","date_gmt":"2015-10-23T06:02:11","guid":{"rendered":"http:\/\/blog.lib.uiowa.edu\/eng\/?p=1177"},"modified":"2017-10-20T14:51:42","modified_gmt":"2017-10-20T19:51:42","slug":"how-many-moles-in-a-mole","status":"publish","type":"post","link":"https:\/\/blog.lib.uiowa.edu\/eng\/how-many-moles-in-a-mole\/","title":{"rendered":"How Many Moles in a Mole?"},"content":{"rendered":"

\"\"<\/a> It is National Mole Day!\u00a0<\/strong><\/p>\n

Sorry\u00a0cute (?), burrowing creature, it isn’t your<\/em> day.<\/p>\n

National Mole Day is celebrated by chemists and chemistry students on October 23rd. The mole\u00a0is honored between 6:02 a.m. and 6:02 p.m. This makes the date 6:02 10\/23,\u00a0And where did that number come from and why does it deserve it’s own day?<\/p>\n

6.02×10^23 is called the Avogadro Constant\u00a0and it defines the number of particles (atoms or molecules) in one mole of substance.<\/p>\n

\"Periodic<\/a>
Periodic Table<\/figcaption><\/figure>\n

The mass of a mole of substance is called the molar mass. The molar mass is used to convert grams of a substance to moles. The molar mass of an element is found on the periodic table, and it is the element’s atomic mass\u00a0in grams\/mole (g\/mol).\u00a0An interactive periodic table can be found here: \u00a0http:\/\/chemistry.about.com\/library\/blperiodictable.htm<\/a>. To explore calculating the mass of a single atom, you will also need to know the atomic mass.\u00a0Want to try calculating an atomic mass? You can find an interactive example here:\u00a0http:\/\/chemistry.about.com\/od\/workedchemistryproblems\/a\/avogadroexampl1.htm<\/a><\/p>\n

In simple terms, a mole of anything is always 6.02×10\u00b2\u00b3. This invented unit is a consistent and convenient measuring unit much like saying a dozen or a byte.<\/p>\n

How to celebrate National Mole Day, you ask?\u00a0<\/strong><\/p>\n

\"Chemistry<\/a>
Chemistry for Today Engineering Library FOLIO QD31.3 .S42 2014<\/a><\/figcaption><\/figure>\n

1.<\/strong> Read a one of our many chemistry books! We have lots of resources, including:<\/p>\n

Corwin, Charles H., Introductory Chemistry : Concepts and Critical Thinking, 7th edition. Boston : Pearson, 2014. Engineering Library FOLIO QD33.2 .C67 2014<\/a><\/p>\n

Seager, Spencer L. Chemistry for Today : General, organic, and biochemistry. Belmont, CA : Brooks\/Cole, 2014. Engineering Library FOLIO QD31.3 .S42 2014<\/a><\/p>\n

2<\/b>. Test your Mole knowledge by taking this quiz<\/a>.<\/p>\n

3<\/b>. Tell mole jokes.<\/p>\n

Where did Avogadro stay on is vacation? A mole-tel.
\nWhat do chemists wear when it’s cold? Ther-mole underwear.<\/p>\n

4.<\/strong> Try a mole experiment<\/a>.<\/p>\n

5.<\/strong> Watch a New York Times science video<\/a> about moles.<\/p>\n

Resources:<\/strong><\/p>\n

Amedeo Avogadro Biography.<\/em> The Famous People<\/a>. Accessed Oct. 22, 2015<\/p>\n

What Is a Mole and Why are Moles Used?<\/em>. 2015. \u00a0About Education.<\/a><\/p>\n

 <\/p>\n","protected":false},"excerpt":{"rendered":"

It is National Mole Day!\u00a0 Sorry\u00a0cute (?), burrowing creature, it isn’t your day. National Mole Day is celebrated by chemists and chemistry students on October 23rd. The mole\u00a0is honored between 6:02 a.m. and 6:02 p.m. This makes the date 6:02 10\/23,\u00a0And where did that number come from and why does it deserve it’s own day?Continue reading “How Many Moles in a Mole?”<\/span><\/a><\/p>\n","protected":false},"author":87,"featured_media":6728,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[5,11],"tags":[],"syndication":[35],"_links":{"self":[{"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/posts\/1177"}],"collection":[{"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/users\/87"}],"replies":[{"embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/comments?post=1177"}],"version-history":[{"count":25,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/posts\/1177\/revisions"}],"predecessor-version":[{"id":6729,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/posts\/1177\/revisions\/6729"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/media\/6728"}],"wp:attachment":[{"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/media?parent=1177"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/categories?post=1177"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/tags?post=1177"},{"taxonomy":"syndication","embeddable":true,"href":"https:\/\/blog.lib.uiowa.edu\/eng\/wp-json\/wp\/v2\/syndication?post=1177"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}