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Moles, Avogadro’s Number, and Molar Mass

Moles, Avogadro’s Number, and Molar Mass. Oh My!!. Definitions. Mole (mol) can be defined as the number equal to the number of carbon atoms in 12.01 grams of carbon (in an chemical equation it is the coefficients that tell how many moles of each compound there are)

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Moles, Avogadro’s Number, and Molar Mass

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  1. Moles, Avogadro’s Number, and Molar Mass Oh My!!

  2. Definitions • Mole (mol) can be defined as the number equal to the number of carbon atoms in 12.01 grams of carbon (in an chemical equation it is the coefficients that tell how many moles of each compound there are) • Avogadro’s number- one mole of something (anything) consists of 6.022 x 1023 units (atoms, molecules, particles, etc…) of that substance • 1 mol = 6.022 x 1023 units • Molar mass- is obtained by summing the masses of the component atoms

  3. examples • 1 mol of Ag= 107.9 amu or g/mol • 1 mol of Ag= 6.022 x1023 atoms • 1 mol of Pb= 207.2 amu or g/mol • 1 mol of Pb= 6.022 x 1023 atoms • Molar mass of CH4 = 16 g (1 C and 4 H) • Molar mass of CaCO3 = 100 g (1 Ca, 1 C and 3 O) • Molar mass of C10H6O3 = 174.1 g (10 C, 6 H, and 3 O)

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