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Daily Science pg. 78

Daily Science pg. 78.

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Daily Science pg. 78

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  1. Daily Science pg. 78 • You are heating copper sulfate in the lab. The mass of your test tube is 13.091g. You add 0.498 g of CuSO4 to the test tube and re-mass the test tube plus the copper sulfate. Your new mass is 13.575 g.After heating the substance for 5 minutes you let it cool and re-mass. The final mass is 13.400 g. What is the formula for the hydrate?

  2. Stoichiometry Pg. 79

  3. Stoichiometry • Chemical reactions stop when one of the reactants has been completely used • As a scientists, we need to know how much that is • Or we might need to know how much product will be made • Stoichiometry tells us this • Stoichiometry: The study of quantitative relationships between amounts of reactants used and products formed

  4. Mole to mass relationships in chemical reactions • Coefficients in an equation tell you how many moles there are of each element • 4 Fe(s) + 3 O2 2Fe2O3 (s) • You can calculate the grams of reactants and products by using stoichiometry (dimensional analysis) • Start with the number of moles of the element and convert to mass using molar mass • Accounts for conservation of mass

  5. Practice Moles to mass • N2 (g) + 3 H2 (g)  2NH3 (g)

  6. Mole to mole ratios • Use the relationships between coefficients to write conversion factors; called mole ratios • 4 Fe(s) + 3 O2 2Fe2O3 (s) • To determine how many mole ratios you can make, multiply the number of reactants and products by the next lowest number

  7. Practice Mole to Mole ratios • 2Al (s) + 3 Br2 (l)  2AlBr3 (s)

  8. Using Stoichiometry – Mole to mole conversions • You must begin with a BALANCED chemical equation • You are given the amount of moles of a substance and you want to know how much of the other reactant you need or how much product will be formed • Start with the given and use mole to mole ratios • Given unit goes on bottom! Desired on top! • Ex. How many moles of hydrogen gas will be produced if you use 0.567 mol of potassium • 2K (s) + 2 H2O (l)  2KOH (aq) + H2 (g)

  9. Practice using mole to mole conversions • How many moles of carbon dioxide are produced when 11.0 moles of propane (C3H8) are burned? • C3H8 (g) + O2 (g)  CO2 (g) + H2O (l)

  10. Pg. 80 • Practice problems pg. 356 1 c-e • Practice problems pg. 357 2 c and 3 a • Practice Problems pg. 359 9 and 10

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