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Understanding Stoichiometry: Calculating Reactant Quantities in Chemical Reactions

This guide explores stoichiometry, the branch of chemistry focused on calculating quantities in chemical reactions. We will illustrate the use of mole ratios derived from balanced equations to determine how much of each reactant is required for a reaction. For instance, when producing 1.5 moles of Fe2O3 from Fe and O2, we'll examine how to calculate the necessary amounts of reactants. Essential mole-mole calculations will be discussed, along with practical examples, such as determining reactant needs when 1.2 moles of oxygen react with excess magnesium.

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Understanding Stoichiometry: Calculating Reactant Quantities in Chemical Reactions

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  1. Stoichiometry • The calculation of quantities using chemical reactions • Example: If we want to make 1.5 moles of Fe2O3 using Fe + O2, how much do we need of the reactants to start?

  2. Mole Ratio • Conversion factor derived from the coefficients of a balanced equation. • It’s the BRIDGE to get across to other elements/compounds

  3. N2 + 3H2 2 NH3 • 1 mole N2 / 3 mole H2 • 2 mole NH3 / 1 mole N2 • 3 mole H2 / 2 mole NH3

  4. Mole-Mole Calculations • Predict products (possible) • Balance equation • Determine mole ratios • Start with what the problem gives you - ALWAYS! • Use the correct mole ratio

  5. Magnesium and oxygen react to form ____________. • How many moles of the product are produced when 1.2 moles of oxygen react with excess magnesium? • How many moles of magnesium reacted in the problem above?

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