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Chapter 12: Stoichiometry

Chapter 12: Stoichiometry. Mr. Samaniego Lawndale High. Problem 12.2 (moles of product). How many moles of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen?. mol = ? (NH 3 ) 0.60 mol N 2. N 2 + H 2 NH 3. 3. 2. 0.60 mol N 2. = 1.2 mol NH 3.

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Chapter 12: Stoichiometry

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  1. Chapter 12: Stoichiometry Mr. Samaniego Lawndale High

  2. Problem 12.2 (moles of product) How many moles of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen? mol = ? (NH3) 0.60 mol N2 N2 + H2 NH3 3 2 0.60 mol N2 = 1.2 mol NH3

  3. 12.1 The Arithmetic of Equations • Balanced equations are necessary to find the amount of product or reactant needed in a chemical reaction. Cu + O2CuO

  4. Problem 12.3 (mass of product) Calculate the number of grams of NH3 produced by the reaction of 5.40 g of hydrogen with an excess of nitrogen. The balanced equation is N2 + H2 NH3 3 2 mass = ? (NH3) 5.40 g H2 5.40 g H2 = 30.4 g NH3

  5. Example Problem (p. 379, 44) Lithium nitride reacts with water to form ammonia and aqueous lithium hydroxide. Li3N + 3H2O NH3 + 3LiOH a. What mass of water is needed to react with 32.9 g of Li3N? b. When the above reaction takes place, how many molecules of NH3 are produced? c. Calculate the number of grams of Li3N that must be added to an excess of water to produce 15.0 L of NH3 (at STP).

  6. Class work • Pages 358-361: 6-14 (skip 11a). (12/14/11, 12/15/11)

  7. Generic Solutions A + B C grams of A to grams of C: grams A  mol A  mol C  grams C mol of A to grams of C: mol A  mol C  grams C mol of A to mol of C: mol A  mol C grams of A to mol of C: grams A  mol A  mol C

  8. Problem 36 b(mass of product) Calculate the number of grams of H2O produced by the reaction of 12.5 g of nitrogen monoxide with an excess of ammonia. The balanced equation is 4NH3 + 6NO 5N2 + 6H2O mass = ? (H2O) 12.5 g NH3 12.5 g NH3 = 19.8 g H2O

  9. Problem 12.4 (molecules of product) After Ch 12 Quiz How many molecules of oxygen are produced when 29.2 g of water is decomposed by electrolysis according to this balanced equation? 2H2O 2H2 + O2 molecules = ? (O2) 29.2 g H2O 29.2 g H2O = 4.88x1023 molecules O2

  10. Problem 12.5 (vol-vol stoichiometry) Nitrogen monoxide and oxygen gas combine to form the brown gas nitrogen dioxide, which contributes to photochemical smog. How many liters of nitrogen dioxide are produced when 34 L of oxygen reacts with an excess of nitrogen monoxide? (Assume @ STP.) vol O2 = 34 L vol = ? (NO2) 2NO + O2 2NO2 34 L O2 Remember: 1 mol = 22.4 L @STP = 68 L NO2

  11. Problem 12.6 (vol stoichiometry) Assuming STP, how many milliliters of oxygen are needed to produce 20.4 mL SO3 according to this balanced equation? 2SO2 + O2 2SO3 vol SO3 = 20.4 mL vol = ? (mL O2) Remember: 1 mol = 22.4 L @STP 20.4 mL SO3 = 10.2 mL O2

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