Ch. 8 Stoichiometry
Title and Highlight TN Ch 8.1 Topic: EQ: Right Side NOTES ONLY Date Write Question out (left side of red line) and answer it (Highlight answer) based on from what you read. Write out the notes from my website. You may use different color pens. Use Bullets or Number notes. Space out your notes so you can add any additional into during lecture. NO HIGHLIGTING, UNDERLINING, etc WE WILL DO OUR FOCUS NOTES TOGETHER Write 2-3 sentences (end of notes) from what you learned from reading, notes, and/or lecture.
Title and Highlight LEFT Side PICTURES, PRACTICE PROBLEMS, ETC TN Ch 8.1 DRAW ANY PICTURES, FIGURES, AND WRITE OUT ANY PRACTICE PROBLEMS/QUESTIONS. WE WILL ANSWER THEM TOGETHER. LEAVE SPACES SO WE CAN ANSWER QUES.
Ch. 8.1-8.3 Topic: Stoichiometry EQ: What is a mole ratio and how is it used in conversions? READ Ch 8.1-8.3 (pg. 249-253) Write Questions & Answer Questions #1, 2a, 3 (notes side) Highlight answer
Stoichiometry refers to the numerical relationship between chemical quantities in a balanced chemical equation.
Interpreting Chemical Equations balance The first thing that must be done is to the equation! N 1 2 (g) + H 3 2 (g) NH 2 3 (g) What are the mole ratios in this equation? Here are the kinds of information you can get from the equation: 1 mole N 2 + 3 moles H 2 2 moles NH 3 1 molecules N 2 + 3 molecules H 2 2 molecules NH 3
Don t draw you already have a copy Stoichiometry Conversion Chart Mass A Mass B Count them Particles A Avogadro s # mole a Molar Mass Count them Mole A Molar Volume Mole Ratio Molar Volume Molar Mass Mole B Count them Avogadro s # mole b Particles B Count them Atoms/Ions in A Volume A Volume Ratio Volume B Atoms/Ions in B
Mole to Mole Conversions The conversion factor is the mole ratio. coefficients The mole ratio comes from the of the balanced chemical equation. Step 1: Write down the known (A) and unknown (B). Step 2: Set up a mole ratio to change from moles A to moles B
Left side - Leave about 5 spaces between each problem Practice Problems: N 2 (g) + 3H 2 (g) 2NH 3 (g) 1) How many moles of ammonia can be made from 7 moles of nitrogen reacting with an excess of hydrogen? 2) How many moles of hydrogen are required to completely react with 8 moles of nitrogen to produce ammonia? 3) How many moles of hydrogen are needed to react with an excess of nitrogen to make 10 moles of ammonia?
Ch. 8.4 Topic: Mole to Mass Conversion EQ: How are mole ratios used in mole-mass conversions? READ Ch 8.4 (pg. 253-257) Write Questions & Answer Questions #4 (notes side) Highlight answer
Left side - Leave about 5 spaces between each problem Practice Problem: CaH 2 (s) + 2H 2 O (l) Ca(OH) 2 (aq) + 2H 2 (g) 1. What mass of calcium hydroxide will be produced from the reaction of 2.50 mol of calcium hydride with excess water? (another product is hydrogen gas) 2. What mass of water is needed?
Mass-Mass Conversion Problems Mass-Mass: (mass A to moles A to moles B to mass B) Step 1: Write down the known (A) and unknown (B). Step 2: Convert from mass A to moles A Step 3: Convert from moles A to moles B using a mole ratio. Step 4: Convert from moles B to mass B.
Left side - Leave about 5 spaces between each problem Practice Problem: 3. How many grams of ammonia can be made from reacting 39.0 grams of nitrogen with an excess of hydrogen? N 2 (g) + 3H 2 (g) 2NH 3 (g)
Ch. 8.5 Topic: Limiting and Excess Reactants EQ: What is the difference between L.R. and E.R.? ***BONUS QUESTION ON EXAM*** READ Ch 8.5 (pg. 257-260) Write Questions & Answer Questions #7 (notes side) Highlight answer
Limiting Reagent (or Limiting Reactant) The limiting reagent is a REACTANT that runs out first. Once the limiting reagent runs out, the rxn stops!! The reactant that is in abundance (reactant that you have too much of) is called the excess reagent.
To summarize: Limiting reactant (or limiting reagent) the reactant that is completely consumed in a chemical reaction. You run out of this reactant first and it stops the rxn. Once you determine LR, that chemical starts every calculation especially THEORETICAL YIELD of product Excess Reactant the reactant you have too much of and have leftovers not being used in the rxn.
Left side - Leave about 10 spaces between each problem Practice Problem #1 2Na(s) + Cl 2 (g) 2 NaCl(s) Know: 53.2 g Na and 65.8 g Cl 2 Find: limiting reactant & theoretical yield of NaCl
Left side - Leave about 10 spaces between each problem Practice Problem #2 Cu 2 O(s) + C(s) 2 Cu(s) + CO(g) Given: 11.5 g Cu 2 O and 114.5 g C Find: limiting reactant & theoretical yield of Cu
Ch. 8.6 Topic: Percent Yield EQ: How do you calculate % yield from actual and theoretical yields? READ Ch 8.6 (pg. 260-264) Write Questions & Answer Questions #8-9 (notes side) Highlight answer
Percent Yield is a ratio that tells us how efficient a chemical reaction is. The higher the % yield, the more efficient the reaction is. (How good is your data!!) % Yield = Percent Yield Actual Yield Theoretical Yield x 100 The actual yield is the amount you experimentally get when you perform the reaction in a lab. (Your result) The theoretical yield is the amount you are ideally supposed to get if everything goes perfectly. (No errors in lab - what you should have got). You can calculate this amount using stoichiometry!
Actual Yield and Percent Yield The Percent yield is always less than 100%. Why??? Errors happen. Some of the product does not form.
Left side - Leave about 10 spaces between each problem Practice Problem #1 USE INFO FROM CH 8.5 TN!! a. Example: 2Na(s) + Cl 2 (g) 2 NaCl(s) Given (grams): 53.2 g Na and 65.8 g Cl 2 Find: limiting reactant and theoretical yield of NaCl. b. Given: actual yield 86.4 g NaCl (PRODUCT) Find: percent yield
Left side - Leave about 10 spaces between each problem Practice Problem #1 USE INFO FROM CH 8.5 TN!! a. Example 8.6: Cu 2 O(s) + C(s) 2 Cu(s) + CO(g) Given (grams): 11.5 g Cu 2 O and 114.5 g C Find: limiting reactant and theoretical yield of Cu b. Given: actual yield 87.4 g Cu Find: percent yield