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Thursday January 31, 2013

Thursday January 31, 2013. ( Mass to Mole Stoichiometry ). Bell Ringer Thursday, 1-31-13. If 5.0 moles of mercury (II) oxide decompose, how many grams of mercury will be produced?. HgO æ Hg + O 2. 2. 2. 5.0 mol. ? grams. 2. mol Hg. 201. g Hg. 5.0 mol HgO. 1005. X. X. =. g Hg. 1.

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Thursday January 31, 2013

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  1. ThursdayJanuary 31, 2013 (Mass to Mole Stoichiometry)

  2. Bell RingerThursday, 1-31-13 • If 5.0 moles of mercury (II) oxide decompose, how many grams of mercury will be produced? • HgOæHg + O2 • 2 • 2 • 5.0 mol • ? grams 2 molHg 201 gHg 5.0 molHgO 1005 X X = gHg 1 2 molHgO 1 molHg

  3. Announcements Happy Inspire Your Heart with Art Day!

  4. Announcements I will be available after school today until 4:45.

  5. Types of Stoichiometry Problems Mass – Mole Conversions: Given is a mass in grams and the unknown is an amount in moles. When you are given the mass of one substance and asked to calculate the amount in moles of another substance in the chemical reaction, the general plan is:

  6. Converting Mass to Moles The following is a solution plan for problems in which the given quantity is expressed in grams and the unknown quantity is expressed in moles.

  7. Converting Mass to Moles Sample Problem The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia: NH3 + O2 → NO + H2O (unbalanced) The reaction is run using 824 g of NH3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H2O are formed?

  8. Converting Mass to Moles Sample Problem The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia: NH3 + O2 → NO + H2O (unbalanced) The reaction is run using 824 g of NH3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H2O are formed? Given: mass of NH3 = 824 g Unknown: a. amt. of NO produced (in mol) b. amt. of H2O produced (in mol)

  9. Converting Mass to Moles Sample Problem The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia: NH3 + O2 → NO + H2O (unbalanced) The reaction is run using 824 g of NH3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H2O are formed? Start with a balanced equation: 4NH3 + 5O2→ 4NO + 6H2O

  10. Converting Mass to Moles Two conversion factors are needed to solve part (a) - the molar mass of NH3 and the mole ratio of NO to NH3. Part (b) starts with the same conversion factor as part (a), but then the mole ratio of H2O to NH3 is used to convert to the amount in moles of H2O. The first conversion factor in each part is the inverted molar mass of NH3.

  11. Converting Mass to Moles Use the periodic table to compute the molar mass of NH3.

  12. Worksheet Mass to Mole Stoichiometry

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