Molar+Mass+and+Mole-Mass+Conversions

**Molar Mass & Mole-Mass Conversions**    media type="custom" key="3841073" **What is a mole, anyway?**   Chemists define a mole as a **collective unit**  that represents  **6.02 x 10 ^ 23 particles of a substance** . Since twenty-one zeros are hard to process, compare the term "mole" to the words "dozen" or "couple." Each are just names for a specific number.

 <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 180%;">**And molar mass?** <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif;"> <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 130%;">The <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(255,0,0); font-size: 130%;">**average atomic mass of an element (expressed in grams)** <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 130%;"> is the molar mass. For example, Gallium's molar mass would be approximately 70 grams because its atomic mass is 69.723 g. <span style="text-align: left; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(115,177,115); font-size: 182%;">

<span style="text-align: left; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(115,177,115); font-size: 182%;"> <span style="color: rgb(255,78,0);"><span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 180%;">**Calculating Compounds** <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif;"> <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 130%;">Figuring out the molar mass of a compound is very similar; a little dimensional analysis is involved, but it all begins with calculating the molar mass of each individual element in the formula.

If there are two or more atoms of a certain element, simply multiply its molar mass by however many atoms there are. Let's try NH3 (Ammonia). Click the link below for a step-by-step demo, and check out our two videos for a more in-depth explanation. <span style="text-align: center; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(0,0,0); font-size: 140.4%;"> [|What is the mass of 90 average sized apples[1.doc]] [|molar mass of glucose[1.doc]]

<span style="text-align: left; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(11,66,11); font-size: 128.7%;"> **<span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif;">And don't forget about significant digits! **

media type="custom" key="3892239" <span style="text-align: left; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(115,177,115); font-size: 182%;"> media type="custom" key="3892207" <span style="color: rgb(255,78,0);"><span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 180%;">**Mole-to-Mass Conversion** <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif;"> <span style="font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; font-size: 130%;">Mole-to-mass conversion is very important, because an experiment may require an exact number of grams (not moles) of a substance. Refer to this equation once you've determined the molar mass of your substance.

<span style="text-align: right; display: block; font-family: 'Palatino Linotype', 'Book Antiqua', Palatino, serif; color: rgb(255,0,0); font-size: 130%;">**mass (grams) = number of moles x __mass (grams)__ 1 mol** media type="custom" key="3897667"

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