chapter 3-6 slides per page - Chemical Reactions and...

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1 TOPICS • Chemical equations • Some simple chemical reactions • Formula weight • The mole • Empirical formulas from analysis • Quantitative information from balanced equations • Limiting reactants Chemical Reactions and Chemical Equations Substances are converted into one or more different substances Reactants: starting materials Products: final materials 2 NaOH + H 2 SO 4 Æ Na 2 SO 4 + 2 H 2 O stoichiometric coefficients subscripts Some Simple Chemical Reactions Combustion: The Mole •M o l e : the amount of substance that contains 6.022x10 23 atoms, or molecules, or formula units, or any entity. • The number 6.022x10 23 is called Avogadro’s number • 1 mole of Cu contains 6.022x10 23 atoms •1 m o l e o f H 2 O contains 6.022x10 23 molecules
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2 Mass – Mole Conversion • Number of moles: n • Mass: m • Molar mass: M Exercise How many moles of mercury(II) sulfate are there in 1.00 kg of this compound? Percent composition of compounds mass % of element X: %X moles of X in formula: n(X) molar mass of X: M(X) molar mass of compound: M Exercise What is the mass % of oxygen in glucose, C 6 H 12 O 6 ? M = 180 g/mol. Empirical Formulas from Analysis Exercise One oxide of iron (Fe) is called magnetite. It is composed of 72.4% Fe and 27.6% O. What is the empirical formula of magnetite? Strategy:
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chapter 3-6 slides per page - Chemical Reactions and...

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