Difference between revisions of "Calculate Molar Mass"
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Atoms are too small to allow meaningful measurement of chemical substances. To work with meaningful amounts of substances, scientists group them into units called moles. A mole is defined as the number of carbon atoms in 12 grams of the isotope carbon-12, which is roughly 6.022 x 10<sup>23</sup> atoms. This number is called Avogadro's number or Avogadro's constant.<ref> http://www.chemteam.info/Mole/MolarMass.html</ref> It is used as the number of atoms for any substance, and the mass of 1 mole of a substance is its molar mass. | Atoms are too small to allow meaningful measurement of chemical substances. To work with meaningful amounts of substances, scientists group them into units called moles. A mole is defined as the number of carbon atoms in 12 grams of the isotope carbon-12, which is roughly 6.022 x 10<sup>23</sup> atoms. This number is called Avogadro's number or Avogadro's constant.<ref> http://www.chemteam.info/Mole/MolarMass.html</ref> It is used as the number of atoms for any substance, and the mass of 1 mole of a substance is its molar mass. | ||
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== Steps == | == Steps == | ||
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#*For glucose, the molar mass is 72.0642 + 12.084 + 95.9964 = 180.1446 g/mol. 180.14 grams is the mass of one mole of glucose. | #*For glucose, the molar mass is 72.0642 + 12.084 + 95.9964 = 180.1446 g/mol. 180.14 grams is the mass of one mole of glucose. | ||
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== Tips == | == Tips == | ||
