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Stoichiometry II

Stoichiometry II. Mole Relationships in Equations. MOLE- MOLE PROBLEMS. Mole-Mole Conversions. How many moles of sodium chloride will be produced if you react 2.6 moles of chlorine gas with an excess (more than you need) of sodium metal?. Flowchart. Atoms or Molecules.

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Stoichiometry II

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  1. Stoichiometry II

  2. Mole Relationships in Equations

  3. MOLE- MOLE PROBLEMS

  4. Mole-Mole Conversions • How many moles of sodium chloride will be produced if you react 2.6 moles of chlorine gas with an excess (more than you need) of sodium metal?

  5. Flowchart Atoms or Molecules Divide by 6.02 X 1023 Multiply by 6.02 X 1023 Moles Multiply by atomic/molar mass from periodic table Divide by atomic/molar mass from periodic table Mass (grams)

  6. Molar Mass of Compounds Molar mass of CaCl2 Calcium = 40.08g Chlorine = 35.45g • Molar Mass of calcium chloride = 40.08 g/mol Ca + (2 X 35.45) g/mol Cl= 110.98 g/mol CaCl2 20 Ca40.08 17Cl 35.45

  7. Calculations molar massGrams Moles Everything must go through Moles!!!

  8. Mole-Mass Conversions 2 Na + Cl2 2 NaCl • Most of the time in chemistry, the amounts are given in grams instead of moles • We still go through moles and use the mole ratio, but now we also use molar mass to get to grams • Example: How many grams of chlorine are required to react completely with 5.00 moles of sodium to produce sodium chloride? 5.00 moles Na 1 mol Cl2 70.90g Cl2 2 mol Na 1 mol Cl2 = 177g Cl2

  9. Practice • Calculate the mass in grams of Iodine required to react completely with 0.50 moles of aluminum.

  10. Mass-Mole • We can also start with mass and convert to moles of product or another reactant • We use molar mass and the mole ratio to get to moles of the compound of interest • Calculate the number of moles of ethane (C2H6) needed to produce 10.0 g of water • 2 C2H6 + 7 O2 4 CO2 + 6 H20 10.0 g H2O 1 mol H2O 2 mol C2H6 18.0 g H2O 6 mol H20 = 0.185 mol C2H6

  11. Mass-Mass Conversions • Most often we are given a starting mass and want to find out the mass of a product we will get (called theoretical yield) or how much of another reactant we need to completely react with it (no leftover ingredients!) • Now we must go from grams to moles, mole ratio, and back to grams of compound we are interested in

  12. Mass-Mass Conversion • Ex. Calculate how many grams of ammonia are produced when you react 2.00g of nitrogen with excess hydrogen. • N2 + 3 H2  2 NH3 2.00g N2 1 mol N2 2 mol NH3 17.06g NH3 28.02g N2 1 mol N2 1 mol NH3 = 2.4 g NH3

  13. Guidelines for Reaction Stoichiometry • Write the balanced equation. • Calculate the number of moles of the species for which the mass is given. • Use the coefficients in the equation to convert the moles of • the given substance into moles of the substance desired. • Calculate the mass of the desired species.

  14. Practice • Calculate how many moles of oxygen are required to make 10.0 g of aluminum oxide

  15. Practice • How many grams of calcium nitride are produced when 2.00 g of calcium reacts with an excess of nitrogen?

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