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Chapter 3

# Chapter 3 - Chapter3:Stoichiometry 1 2 3 4 5 6 7 8...

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Chapter 3:  Stoichiometry 1. Atomic Mass 2. Moles and Molar Mass 3. Percent Composition of Compounds 4. Empirical & Molecular Formulas of Compounds 5. Writing and Balancing Chemical Equations 6. Stoichiometry 7. Limiting Reactants 8. Reaction Yields

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Mass Spectrometer  (Figure 3.1)
Mass Spectrometer Signal for Neon   (Figure 3.2)

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Example 1     The element rhenium (Re) has only two  naturally occurring isotopes,  185 Re and  187 Re,  with an average atomic mass of 186.207 amu.   The atomic mass of  185 Re is 184.953 amu  and the atomic mass of  187 Re is 186.956 amu.   Find the natural abundance of each isotope.      Answer: 62.6%  187 Re and 37.4%  185 Re
Example 2 What is the mass of 1.00 mole of methane,  CH 4 ?     Answer: 16.0 g

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Example 3 How many moles of K 2 SO 4  are present in  10.0 g of this substance? Answer:  0.0574 moles of K 2 SO4
Example 4 How many moles of O atoms are present in  5.40 g of H 2 O 2 ?  How many O atoms is  that? Answer:  0.318 moles of O; 1.91x10 23   atoms of O

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Example 5 What is the mass of 2.75 moles of H 3 PO 4 ? Answer:  269 g
Example 6 What is the mass of one helium atom, on  average, in grams?

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