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Chemical Quantities

Chemical Quantities. Chapter 10. Molar Mass. Molar mass is the sum of atomic masses of the elements in the compound. You MUST take into account the number of atoms of each element. Example: Ca 3 (PO 4 ) 2 Ca 3(40.08) P 2(30.97) +O 8(16.00) 310.18 g Ca 3 (PO 4 ) 2

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Chapter 7 Section 3 and 4

Chapter 7 Section 3 and 4. Percent composition Empirical Formula Molecular Formula. Calculating Formula Mass. Calculate the formula mass of magnesium carbonate, MgCO 3 . 24.31 g + 12.01 g + 3(16.00 g) =. 84.32 g. Calculating Percentage Composition.

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Empirical vs. molecular

Empirical vs. molecular. Empirical formula. Is the simplest form of a formula Is written in the lowest possible ratio E.g., CH 2 O or CH Will be reduced. May or may not exist in this form in the real world. Molecular formula.

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381 views • 19 slides

Calculating Empirical and Molecular Formulas

Calculating Empirical and Molecular Formulas. A chemical formula in which the ratio of the elements are in the lowest terms is called an empirical formula . For example, the empirical formula for a glucose molecule (C 6 H 12 O 6 ) is CH 2 O. All the subscripts are

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595 views • 12 slides

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True formula - PowerPoint PPT Presentation

Chemical Quantities

Chapter 7 Section 3 and 4

Empirical vs. molecular

Calculating Empirical and Molecular Formulas