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Stoichiometry – Chapter 12

Stoichiometry – Chapter 12. Stoichiometry. We are going to use the ‘mole’ to convert from one substance to another substance. You need to look at a balanced chemical reaction in order to determine the molar ratio between 2 substances. Stoichiometry.

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Stoichiometry – Chapter 12

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  1. Stoichiometry – Chapter 12

  2. Stoichiometry We are going to use the ‘mole’ to convert from one substance to another substance. You need to look at a balanced chemical reaction in order to determine the molar ratio between 2 substances.

  3. Stoichiometry 4HNO3 (aq) + Sn (s) SnO2 (s)+ 4NO2 (g) + 2H2O (l) You need to look at a balanced chemical reaction in order to determine the molar ratio between 2 substances.

  4. Stoichiometry 4HNO3 (aq) + Sn (s) SnO2 (s) + 4NO2 (g) + 2H2O (l) Molar ratios: 4 mole HNO34 mole HNO3 1 mole Sn1 mole SnO2 4 mole NO34 mole NO31 mole Sn1 mole Sn 4 mole NO2 2 mole H2O 1 mole SnO2 4 mole NO2 1 mole Sn1 mole SnO21 mole SnO2 * You can also use the 2 mole H2O 4 mole NO2 2 mole H2O the inverse of these. *

  5. Stoichiometry Write all of the molar ratio’s from the following chemical reaction; C25H52(g) + 38O2(g)  25CO2(g) + 26H2O(g)

  6. Stoichiometry 4HNO3 (aq) + Sn (s) SnO2 (s) + 4NO2 (g) + 2H2O (l) Calculate the mass of water produced if 10.00 grams of nitric acid is allowed to react. Calculate the mass of nitrogen dioxide produced if 10.00 grams of nitric acid reacted.

  7. Stoichiometry Limiting Reactants Eventually, one of the reactants will be used up first. This reactant is called the limiting reactant. To determine which reactant is limiting, calculate the theoretical amount of product you should produce. The reactant that produces the least amount of reactant is the limiting reactant.

  8. Stoichiometry Limiting Reactants H2O (l) + CO2(g) H2CO3(aq) If 5.00 grams of H2O is allowed to react with 2.50 grams of CO2, what is the maximum amount of H2CO3 that could be produced? Which is the limiting reactant?

  9. Stoichiometry Limiting Reactants CaCl2(aq) + Na2CO3(aq) 2NaCl (aq) + CaCO3(s) What mass of NaCl would be produced if 1.0 kg of each reactant is used to produce sodium chloride and calcium carbonate? Which is the limiting reactant? Calculate the mass of the non-limiting reactant.

  10. Stoichiometry Reagents in Excess A reactant that is not used-up completely in a chemical reaction is called the reagent in excess. 4Na (s) + O2(g) 2Na2O (s) What mass would remain of the reagent in excess if 0.60 moles of Na is placed in a reaction vessel that contains 1.0 L of O2 at STP?

  11. Stoichiometry Calculating Percent Yield There are many factors that affect the yield of a product in a chemical reaction. Pressure, temperature, volume, catalysts, and closed systems all affect the amount of product that is produced in a chemical reaction. The Percent Yield of a chemical reaction is the amount of product that was recovered as a percentage of the theoretical amount that should have been produced.

  12. Stoichiometry Calculating Percent Yield TheTheoretical Yield of a chemical reaction is the amount of product that should be produced given that all of the limiting reactant will allow % Yield = Amount Recovered x 100 Theoretical Yield

  13. Stoichiometry Calculating Percent Yield 4Na (s) + O2(g) 2Na2O (s) Calculate the theoretical yield of Na2O if 5.00 grams of Na is added to 7.50 grams of O2.

  14. Stoichiometry Calculating Percent Yield 4Na (s) + O2(g) 2Na2O (s) Calculate the percent yield of the reaction if 6.00 grams of Na2O was recovered.

  15. Stoichiometry Calculating Percent Yield Ca(NO3)2(aq)+ NaCO3(aq) 2NaNO3(aq) +CaCO3(s) 2.00 g of Ca(NO3)2is added to 3.00 g of NaCO3. 0.750 g of the precipitate was isolated from the chemical reaction. What is the percent yield of this chemical reaction?

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