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Chapter 12 Stoichiometry part 1

Chapter 12 Stoichiometry part 1. Stoichiometry. The study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry. Calculations of quantities in chemical reactions

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Chapter 12 Stoichiometry part 1

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  1. Chapter 12 Stoichiometrypart 1

  2. Stoichiometry The study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction

  3. Stoichiometry • Calculations of quantities in chemical reactions • This means using balanced equations to calculate quantities of chemicals used in a chemical reaction

  4. Law of Conservation of Mass • Matter is neither created nor destroyed in a chemical reaction • Chemical bonds in reactants break and new chemical bonds form to produce products • Mass of reactants equals the mass of the products

  5. A chemical equation is like a recipe; it shows you how much of each “ingredient” is used and how much product you will have in the end.

  6. The heart of stoichiometry is using a balanced chemical equation as a conversion factor for dimensional analysis.

  7. N2 + 3H2 2NH3 • How many molecules of N2 are there? • How many molecules of H2 are there? • How many molecules of NH3 are there? So one molecule of N2 will react with 3 molecules of H2 to form 2 molecules of NH3. You could also say that one mole of N2 will react with 3 moles of H2 to form 2 moles of NH3.

  8. This equation tells the proportions of N2, H2, and ammonia • The coefficients are in a 1:3:2 ratio • The ratio could mean molecules or moles of each

  9. Review 6.02 x 1023 particles 1 mole molar mass 1N2(g) + 3H2(g)  2NH3(g)‏ 1 mole 3 moles 2 moles 28.00g 3(2.02)=6.06g 2(14.00+3.03)=34.06g

  10. Steps to solve every problem: • Write a balanced equation. • Put what you have over 1. • Convert into moles. • Compare using the equation. • Convert into the unit the question asks for.

  11. Mole to Mass conversion: Mole to Mole conversions: Conversion factor (as with any conversion factor, units must cancel) Moles of known x moles of unknown = moles unknown Moles of known The mole ratios of the balanced equation is known, and you’re given a quantity in moles, now find the mass of another product or reactant.

  12. Burning of propane gas:C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) How much oxygen is needed to produce 18 mol of CO2?

  13. Zn + HCl  ZnCl2 + H2 • For the above reaction, how many moles of zinc chloride can be produced with 0.27 moles of zinc? • For the above reaction, how many moles of zinc will react with 1.39 moles of hydrochloric acid?

  14. Fe + O2 Fe2O3 • How many grams of iron (III) oxide can be produced with 17.2g Fe? • How many molecules of O2 are needed to produce 3.92g Fe2O3?

  15. Mass to Mass conversion: Again, the mole ratios of the balanced equation is known and you’re given a quantity in grams, now find the mass of another product or reactant. C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) 67.02g propane would produce ? grams of water vapor?

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