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Compound Stoichiometry Unit 5 What Is Stoichiometry?

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Compound Stoichiometry Unit 5 What Is Stoichiometry? Compound Stoichiometry Unit 5 What is Stoichiometry? Compound vs Reaction Stoichiometry Molecular Mass Hydrate problems Moles and Avagadro’s Number Percentage Composition Problems Empirical Formula Problems Molecular Formula Problems Hydrates again Stoichiometry Stoichiometry: Element measurement Stoichiometry problems involve calculations (you will need a calculator for this) 2 types of Stoichiometry Problems Compound Stoichiometry Reaction Stoichiometry Types of Compound Stoichiometry Problems Formula/ Molecular Mass Problems Mole Problems Avogadro’s Number Problems Percentage Composition Problems Empirical Formula Problems Molecular Formula Problems Formula/Molecular Mass How to find Formula/Molecular Mass of a compound: write a correct formula for the compound Round the average atomic mass (on periodic table) -round to the nearest whole number- Multiply the Rounded atomic mass of each element but the number of atoms of that element present (usually subscripted) Add the total rounded atomic masses of all elements in the compound and label it with amu: Atomic Mass Units Ex 5-1: Formula/Molecular Mass Problems Find the formula mass of Calcium Phosphate: Ca3(PO4)2 Element # * AMU AMU Ca 3 * 40 = 120 P 2 * 31 = 62 O 8 * 16 = 128 Total AMU: 310 amu Ex 5-2: Find the formula mass of ammonium sulfate: (NH4)2SO4 Ex 5-3: Find the Molecular Mass of dichloride heptoxide: Hydrates Hydrates are ionic compounds which trap water molecules in their crystal structures Need to know how to name and recognize hydrates Formula: Ionic Compound * # H20 Naming: Name your Ionic Compound add a numerical prefix tot he word hydrate Ex: CuSO4 * 5 H2O copper (II) pentahydrate Hydrates Formula Mass Add all the average atomic mass of the ionic compound together Add the mass of the # of H2O (18 amu) 5 H2O = 80 amu Add both the atomic masses of the ionic compound and H2O Ex 5-5: Find the formula mass of barium chlorate hexahydrate Ba(ClO3)2 * 6 H2O Moles A mole is a unit in chemistry that indicates a definite number of particles Just as a “dozen” is a universal unit in America for 12 a mole is the chemist’s universal unit for number of particles 1 mole = 6.022 * 1023 representative particles (Avogadro’s number) What is a representative particle? More Moles Elements (except diatomic) the representative particle is the Atom 1 mole of Aluminum = 6.022 *1023 Atoms of Aluminum For diatomic and compounds the representative particles is the Molecules 1 mole of CO2 = 6.022 * 1023 molecules of CO2 1 mole of O2 = 6.022 * 1023 molecules of O2 Even More Moles Ionic compounds the representative particles are formula units 1 mole NaCl = 6.022 * 1023 Formula Units Whats the point of all this? No matter what kind of compound and its overall weight it contains the same number of representative particles Periodic Table: the amu is the amount of grams to make 1 mole of that substance H2O = 18 amu = 1 mole of H2O So H2O also has 18 g per 1 mole of H2O (helps when converting) Ex 5-6: I have 200 grams of Calcium Carbonate, How many moles of Calcium Carbonate do I have: What if I had 300 g of Calcium Carbonate: What if I had 50 g of Calcium Carbonate: What if I had 63.2 g of Calcium Carbonate: Calculating Moles Tips 2 ways of calculating moles Formula: Moles = Mass of a substance (grams) / formula mass of substance Dimensional analysis Ex 5-7: How many moles are in 28.7 grams of Lithium Nitrate LiNO3 = 69 g/mole By Equation: Mole = mass / mw 28.7 g / (69 g/mol) .416 mol of LiNO3 Dimensional Analysis: 28.7 g 1 Mole X .416 mol LiNO3 69 g Ex 5-8: How many Moles are in 100 g of water? Ex 5-9: How many moles of iodine are there in 200 grams of Iodine? Hint: Iodine is a Diatomic Ex 5-10: If 47.4 grams of an ionic compound are known to be 1.185 moles of that compound what is the formula mass of that compound? Ex 5-11: If 256 grams of a pure monatomic element are known to be 8.26 moles of that element what element are we talking about? Ex: 5-12: How many grams of water are in 1.34 moles of water? Avogadro’s Number Problems: Avogadro’s Number ( 6.022 * 1023) Represents particles in 1 mole of a substance non-diatomic element have 6.022 * 1023 atoms in 1 mole of that same element In diatomic molecules remember they are represented with 2 moles per element “set” so it would be 6.022 * 1023 atoms in 1 mole of that same element Avogadro's Number Problems The atomic mass of 65 amu. This means that one mole of zinc weights 65 grams There are also 6.022 * 1023 atoms of zinc in 65 grams (1 mole) of zinc. Avogadro's Number Problems IF the atomic mass of water is 18 g/mole that means that there are 6.022 * 1023 molecules of water in 18 grams of it or 1 mole of it. Avogadro's Number Problems Representative particles of Elements are represented in Atoms Representative particles of molecular compounds (2+nonmetals) are molecules Representative particles of an ionic compound is called Formula units When in Doubt GO TO MOLES!!! Ex 5-13: How many atoms are present in pure iron nail which weighs 13.2 g? Ex 5-14: If there are known to be 8.24 *1026 molecules of water present, would the sample of water weigh more then a pound? 1lb = 454 g Ex 5-15: How many moles of Carbon dioxide are 24 present in 4.55 * 10 molecules of CO2? Ex 5-16: How many formula units are there in 7.55 grams of sodium sulfate? Ex 5-17: If I know that a sample of mercury (II) chloride contains 7.32 * 1024 formula units how much does the sample weight in pounds? 1 lb = 454 g Example 5-18: Which would contain more representative particles 46 grams of Sodium Hydroxide or 46 grams of Carbon Dioxide? Example 5-19: Which weighs more 6.24 * 1023 formula units of sodium bromide or 6.24 * 1024 molecules of phosphorus tribromide? Percent Composition Problems You are comparing the parts to the hole numbers Percent composition is base on mass not atoms present We are going to find the percentage BY MASS of certain elements in a compound by comparing the mass of the element to the mass of the entire compound How to find Percentage Composition 1.Write a correct formula for the compound in the question 2.Find the formula or molecular mass of the entire compound 3.Divide the total mass of the Element whose percentage you are looking for by the total mass of the entire compound 4.Multiply your result by 100 to convert to a percentage 5.Express your answer to 1 decimal place and add a % sign at the end Example 5-20: What is the COMPLETE percentage composition (by mass) of Potassium Dichromate ? Percentage of Each Element Example 5-20 What is the percentage of Calcium in Calcium Phosphide? Example 5-21: What is the percent of oxygen in barium chlorate hexahydrate? Percentage Composition % s are excellent conversion factor since it represents a comparison of units to 100 units The next problems can be worked using dimensional analysis or by finding the % of a particular element present and then multiplying it times the mass of the compound given Example 5-22: How many grams of of Calcium are present in 156.8 g of chalk? (Calcium Carbonate) Example 5-23: How many grams of pure iron can be recovered from 50 grams of iron ore which is known to contain 32% Iron (II) Nitrate? Example 5-24:Lime stone is known to be 95% calcium carbonate. How many grams of pure calcium could you expect to obtain from a piece of lime stone weighing 100 kg? Empirical Formula Problems Empirical Formula - shows the ratio of the smallest amount of atoms in a compound RATIO OF THE ATOMS PRESENT (CH2O) The Ratio tells us how many of each atom is present To solve empirical you must be given either the grams of each element present or the % of each element present How to solve Empirical Formula Problems 1.Divide either the % of each element OR the Grams of each element Given by the atomic mass of the element. Leave your answer in 4 sig figs for accuracy 2.Compare the results you got in step 1 by selecting the smallest of the results and dividing all of the results by the smallest value. You should get a result which is very close to a whole number or very close to a mix number which contains a recognizable fraction ( 1/3 = .3333) How to solve Empirical Formula Problems 3. If All results in #2 are whole number use them as subscripts and write the formula out. If all results in # 2 are not whole numbers you must multiply all the results in #2 by a number that will make all the numbers whole numbers (ex 1.5 * 2 = 3) 4.Write the metal first (if there is one) If there is a list of elements then list them in alphabetical order. Example 5-25: A compound is found to contain 10.14% lithium, 20.29% nitrogen and 69.57% oxygen. What is the empirical formula of the compound? Example 5-26 A 200 gram sample of a compound which contain only carbon, hydrogen and oxygen is found to contain: 94.74 grams of carbon, 21.05 grams of hydrogen, and 84.21 grams of Oxygen.
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