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1 The Mole **Make sure you get your daily work signed off on. That way, when we test you'll have the grade you earned instead of Videos freaking out about 50's in the book. #1 -- The Mole #2 -- Particles Per Mole Video NAME: #3 -- Molar Mass Conversion Video PERIOD: #4 -- Percent Composition Video #5 -- Calculating Empirical Formula Practice Problems: Practice Sheets: pg 86 Gram/Mole Conversions Grams to Mole Calculations pg 87 Gram/Mole Conversions Molar Mass Calculations pg 88 Conversions with Avagadro's number Mole Calculations Wkst pg 233 Molar Mass Moles/Molecules/Grams Conversions pg 234 Molar mass as a conversion factor Moles Practice pg 235 Molar mass as a conversion factor pg 237 Percent composition pg Emperical formulas pg 242 Molecular formulas Labs: Activities: Quizzes: Chalk Lab Bubble Gum Lab Mole Lab the Works Mole Airlines Flight Ebola Mole Particles per mole Gram mole conversions Molar mass as conversion factor. Percent composition Empirical and Molecular Formulas

2 0THE MOLE How many molecules would be in 3 moles of water? The mole (mol) is one of the seven base units in the SI system. It measures the. The form in which a substance exists is its. Representative particles can be atoms, ions, molecules, formula units, or anything else. Just as a dozen is 12 representative particles, a mole is representative particles. Ex. 1 mole Fe atoms = 6.02 x atoms of Fe 1 mole H2O molecules = 6.02 x molecules of water 1 mole NaCl formula units = 6.02 x NaCl formula units 1 mole eggs = 6.02 x eggs Write the memory tricks for remembering diatomic elements. Diatomic Elements Certain elements are only stable in pairs or with other elements in a compound. These elements are called the. There are 7 diatomic elements:,,,,,, (Memory trick: or ) Avogadro s Number 6.02 x is called Avogadro s number. It is named after Amadeo Avogadro who did work in the 1800 s that allowed 6.02 x to be calculated. The mole is the chemist s dozen. It is a convenient way to count extremely large numbers of atoms, molecules or ions. New Conversion Factor! 1 mole = 6.02 x representative particles We work these problems using dimensional analysis. Your friend gives you a gold ring that contains 2.3 mol of atoms. How many atoms is this? Examples: How many moles are 1.20 x atoms of phosphorous? How many atoms are in mol of Zn? How many molecules are in mol N2O5? How many moles are contained in 1.20 x molecules CO2?

3 Gram atomic mass (gam) atomic mass of an in grams -mass of one mole of atoms of a monatomic element -use the periodic table and take masses to 0.1 g Ex. C = 12.0 g = mass of atoms 12.0 g/mol is the gram atomic mass of There are two terms to describe the mass of a chemical compound; gram molecular mass or gram formula mass. We will most often use the term gram formula mass. Molar mass or are terms also used to mean the same thing. What is the gram molecular mass of P2O5? Gram molecular mass (gmm) mass of one mole of a -sum of the atomic masses of each atom in the molecule Ex. 1 mol H2O: 2 mol H =2 x 1.0 g H/mol = 2.0 g 1 mol O =1 x 16.0 g O/mol = 16.0 g 18.0 g H2O Example What is the gram molecular mass of CH3OH? Gram formula mass (gfm) -mass of one mole of an compound -sum of the atomic masses of each atom in a formula unit Example What is the gfm of magnesium phosphate (Mg3(PO4)2)? What is the molar mass of ammonium sulfate ((NH4)2SO4)? Write the two conversion factors we have discussed below. Show how they are related. Mole Mass Conversions New Conversion factor! 1 mol = gfm Find the mass in grams of 3.32 mol of K mol K =? g K Conversion factor: 1 mol K = 39.1 g (from periodic table) Use dimensional analysis: 3.32 mol K 39.1 g K = 1.30 x 10 2 g K 1 mol K Find the mass in grams of 15.0 mol of sulfuric acid (H2SO4). Find the number of moles in 11.0 g of methane (CH4).

4 MULTI-STEP MOLE PROBLEMS: Calculate the number of molecules present in 4.29 g of nitrogen dioxide (NO2). Calculate the number of moles of sulfur atoms present in 2.01g of sodium sulfide (Na2S). Calculate the mass in grams of 2.49 x carbon dioxide (CO2) molecules. Calculate the grams of carbon in 12.2 mol of sucrose, C12H22O11. Relate the three conversion factors we have learned below. Molar Volume of a Gas The volume of a gas is usually measured at and atmosphere of pressure. This is called standard temperature and pressure (STP). At STP, one mole of any gas has a volume of 22.4 L L is called the molar volume of a gas L of a gas at STP contains 6.02 x particles of the gas L of a gas has a mass equal to the gfm of the gas. New conversion factor! 1 mol of any gas at STP = 22.4 L (for gases only) What is the volume (liters) at STP of mol of methane, CH4? mol =? L At STP, how many moles are in ml of neon gas? Percent Composition

5 (remember: percent = ) -percent by mass of in a compound Two types of problems: Find the % composition for a compound that is formed from 28.0 g Fe and 8.0g O. What is the percent composition of calcium acetate (Ca(C2H3O2)2)? % mass = grams of element x 100 gfm of compound CALCULATING EMPIRICAL FORMULAS Empirical formula formula that represents the lowest of the various types of atoms in a compound Steps to calculate empirical formula: 1. Find the mass of each element in a sample of the compound 2. Convert the mass to moles of each element 3. Simplify mole ratio (divide each mass by the smallest mass to get ratios of each element). 4. If your answers are not in whole numbers, you must multiply by 2,3,4,or 5 to get whole numbers. 5. Use mole ratio as subscripts in the formula If given % composition, assume 100 g of compound. A compound is 79.8% C and 20.2% H. Find its empirical formula. Empirical Formula Poem Percent to mass, Mass to mole, Divide by smallest, Round (or multiply) till whole Find the empirical formula for a compound made up of 26.7% P, 12.1% N and 61.2%Cl.

6 Finding Molecular Formulas Molecular formulas are the formulas. They may be the same as the empirical formula or a multiple of it. To find the multiple (n), take the gram formulas mass (gfm) and divide by the n = gfm efm Multiply each subscript in the empirical formula by n to get the molecular formula. A white powder is analyzed and found to have the empirical formula P 2 O 5. The compound has a molar mass of g. What is the compound s molecular formula? A compound used as an additive for gasoline to help prevent engine knock shows the following percentage composition: 71.65% Cl 24.27% C 4.07% H The molar mass is known to be g. Determine the empirical formula and the molecular formula for this compound.

7 Grams/Moles Calculations Given the following, find the number of moles: 1) 30 grams of H 3 PO 4 2) 25 grams of HF 3) 110 grams of NaHCO 3 4) 1.1 grams of FeCl 3 5) 987 grams of Ra(OH) 2 6) 564 grams of copper 7) 12.3 grams of CO 2 8) 89 grams of Pb(CH 3 COO) 4 WKS001x Cavalcade Publishing ( All Rights Reserved

8 Given the following, find the number of grams: 9) 4 moles of Cu(CN) 2 10) 5.6 moles of C 6 H 6 11) 21.3 moles of BaCO 3 12) 1.2 moles of (NH 4 ) 3 PO 3 13) 9.3 x 10-3 moles of SmO 14) 6.6 moles of ZnO 15) 5.4 moles of K 2 SO 4 16) 88.4 moles of NI 3 WKS001x Cavalcade Publishing ( All Rights Reserved

9 Grams/Moles Calculations Answer Key Given the following, find the number of moles: 1) 30 grams of H 3 PO moles 2) 25 grams of HF 1.25 moles 3) 110 grams of NaHCO moles 4) 1.1 grams of FeCl moles 5) 987 grams of Ra(OH) moles 6) 564 grams of copper 0.11 moles 7) 12.3 grams of CO moles 8) 89 grams of Pb(CH 3 COO) moles Given the following, find the number of grams: 9) 4 moles of Cu(CN) grams 10) 5.6 moles of C 6 H grams 11) 21.3 moles of BaCO grams 12) 1.2 moles of (NH 4 ) 3 PO grams 13) 9.3 x 10-3 moles of SmO 1.5 grams 14) 6.6 moles of ZnO grams 15) 5.4 moles of K 2 SO grams 16) 88.4 moles of NI grams WKS001x Cavalcade Publishing ( All Rights Reserved

10 Molar Mass Worksheet Calculate the molar mass of the following chemicals: 1) Cl 2 2) KOH 3) BeCl 2 4) FeCl 3 5) BF 3 6) CCl 2 F 2 7) Mg(OH) 2 8) UF 6 9) SO 2 10) H 3 PO 4 11) (NH 4 ) 2 SO 4 12) CH 3 COOH 13) Pb(NO 3 ) 2 14) Ga 2 (SO 3 ) 3 WKS001x Cavalcade Publishing ( All Rights Reserved

11 Molar Mass Worksheet Answer Key Calculate the molar mass of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl g/mol 5) BF g/mol 6) CCl 2 F g/mol 7) Mg(OH) g/mol 8) UF g/mol 9) SO g/mol 10) H 3 PO 4 98 g/mol 11) (NH 4 ) 2 SO g/mol 12) CH 3 COOH 60 g/mol 13) Pb(NO 3 ) g/mol 14) Ga 2 (SO 3 ) g/mol WKS001x Cavalcade Publishing ( All Rights Reserved

12 Mole Calculation Worksheet 1) How many moles are in 15 grams of lithium? 2) How many grams are in 2.4 moles of sulfur? 3) How many moles are in 22 grams of argon? 4) How many grams are in 88.1 moles of magnesium? 5) How many moles are in 2.3 grams of phosphorus? 6) How many grams are in 11.9 moles of chromium? 7) How many moles are in 9.8 grams of calcium? 8) How many grams are in 238 moles of arsenic? What are the molecular weights of the following compounds? 9) NaOH 12) H 3 PO 4 10) H 2 O 13) Mn 2 Se 7 11) MgCl 2 14) (NH 4 ) 2 SO 4 WKS01x Cavalcade Publishing ( All Rights Reserved

13 15) How many grams are in 4.5 moles of sodium fluoride, NaF? 16) How many moles are in 98.3 grams of aluminum hydroxide, Al(OH) 3? 17) How many grams are in 0.02 moles of beryllium iodide, BeI 2? 18) How many moles are in 68 grams of copper (II) hydroxide, Cu(OH) 2? 19) How many grams are in 3.3 moles of potassium sulfide, K 2 S? 20) How many moles are in 1.2 x 10 3 grams of ammonia, NH 3? 21) How many grams are in 2.3 x 10-4 moles of calcium phosphate, Ca 3 (PO 3 ) 2? 22) How many moles are in 3.4 x 10-7 grams of silicon dioxide, SiO 2? 23) How many grams are in 1.11 moles of manganese sulfate, Mn 3 (SO 4 ) 7? WKS01x Cavalcade Publishing ( All Rights Reserved

14 Mole Calculation Worksheet Answer Key 1) How many moles are in 15 grams of lithium? 0.46 moles 2) How many grams are in 2.4 moles of sulfur? 77.0 grams 3) How many moles are in 22 grams of argon? 0.55 moles 4) How many grams are in 88.1 moles of magnesium? 2141 grams 5) How many moles are in 2.3 grams of phosphorus? moles 6) How many grams are in 11.9 moles of chromium? grams 7) How many moles are in 9.8 grams of calcium? 0.24 moles 8) How many grams are in 238 moles of arsenic? 17,826 grams What are the molecular weights of the following compounds? 9) NaOH 40.1 grams 12) H 3 PO grams 10) H 2 O 18.0 grams 13) Mn 2 Se grams 11) MgCl grams 14) (NH 4 ) 2 SO grams 15) How many grams are in 4.5 moles of sodium fluoride, NaF? 189 grams 16) How many moles are in 98.3 grams of aluminum hydroxide, Al(OH) 3? 1.26 moles 17) How many grams are in 0.02 moles of beryllium iodide, BeI 2? 5.2 grams 18) How many moles are in 68 grams of copper (II) hydroxide, Cu(OH) 2? 0.70 moles 19) How many grams are in 3.3 moles of potassium sulfide, K 2 S? grams 20) How many moles are in 1.2 x 10 3 grams of ammonia, NH 3? 70.6 moles 21) How many grams are in 2.3 x 10-4 moles of calcium phosphate, Ca 3 (PO 3 ) 2? grams 22) How many moles are in 3.4 x 10-7 grams of silicon dioxide, SiO 2? 5.66 x 10-9 moles 23) How many grams are in 1.11 moles of manganese sulfate, Mn 3 (SO 4 ) 7? grams WKS01x Cavalcade Publishing ( All Rights Reserved

15 Moles, Molecules, and Grams Worksheet 1) How many molecules are there in 24 grams of FeF 3? 2) How many molecules are there in 450 grams of Na 2 SO 4? 3) How many grams are there in 2.3 x atoms of silver? 4) How many grams are there in 7.4 x molecules of AgNO 3? 5) How many grams are there in 7.5 x molecules of H 2 SO 4? 6) How many molecules are there in 122 grams of Cu(NO 3 ) 2? 7) How many grams are there in 9.4 x molecules of H 2? 8) How many molecules are there in 230 grams of CoCl 2? WKS001x Cavalcade Publishing ( All Rights Reserved

16 9) How many molecules are there in 2.3 grams of NH 4 SO 2? 10) How many grams are there in 3.3 x molecules of N 2 I 6? 11) How many molecules are there in 200 grams of CCl 4? 12) How many grams are there in 1 x molecules of BCl 3? 13) How many grams are there in 4.5 x molecules of Ba(NO 2 ) 2? 14) How many molecules are there in 9.34 grams of LiCl? 15) How many grams do 4.3 x molecules of UF 6 weigh? 16) How many molecules are there in 230 grams of NH 4 OH? WKS001x Cavalcade Publishing ( All Rights Reserved

17 Moles, Molecules, and Grams Worksheet Answer Key 1) How many molecules are there in 24 grams of FeF 3? 1.28 x molecules 2) How many molecules are there in 450 grams of Na 2 SO 4? 1.91 x molecules 3) How many grams are there in 2.3 x atoms of silver? 421 grams 4) How many grams are there in 7.4 x molecules of AgNO 3? 209 grams 5) How many grams are there in 7.5 x molecules of H 2 SO 4? 122 grams 6) How many molecules are there in 122 grams of Cu(NO 3 ) 2? 3.92 x molecules 7) How many grams are there in 9.4 x molecules of H 2? 312 grams 8) How many molecules are there in 230 grams of CoCl 2? 1.07 x molecules 9) How many molecules are there in 2.3 grams of NH 4 SO 2? 1.69 x molecules 10) How many grams are there in 3.3 x molecules of N 2 I 6? 430 grams 11) How many molecules are there in 200 grams of CCl 4? 7.82 x molecules 12) How many grams are there in 1 x molecules of BCl 3? 195 grams 13) How many grams are there in 4.5 x molecules of Ba(NO 2 ) 2? 17.1 grams 14) How many molecules are there in 9.34 grams of LiCl? 1.33 x molecules 15) How many grams do 4.3 x molecules of UF 6 weigh? 2.51 grams 16) How many molecules are there in 230 grams of NH 4 OH? 3.96 x molecules WKS001x Cavalcade Publishing ( All Rights Reserved

18 Mole Problem Using your knowledge of mole calculations and unit conversions, determine how many atoms there are in 1 gallon of gasoline. Assume that the molecular formula for gasoline is C 6 H 14 and that the density of gasoline is approximately 0.85 grams/ml. There are atoms in 1 gallon of gasoline Cavalcade Publishing For chemistry help, visit

19 Mole Problem Solution Using your knowledge of mole calculations and unit conversions, determine how many atoms there are in 1 gallon of gasoline. Assume that the molecular formula for gasoline is C 6 H 14 and that the density of gasoline is approximately grams/ml. Using a conversion factor of 3785 ml per gallon, we can determine that the mass of gasoline in one gallon is 3785 ml x g/ml = 3217 grams. Because the molar mass of C 6 H 14 is 86 g/mole, there are 3217 / 86 moles of gasoline molecules, or 37.4 moles of molecules present. Multiplying 37.4 x 20 (the number of atoms per mole of gasoline), there are 748 moles of atoms. Finally, multiplying 748 moles of atoms by 6.02 x atoms/mole, we can find that there are 4.50 x atoms present in the sample. There are 4.50 x atoms in 1 gallon of gasoline Cavalcade Publishing For chemistry help, visit

20 Moles Worksheet 1) Define mole. 2) How many moles are present in 34 grams of Cu(OH) 2? 3) How many moles are present in 2.45 x molecules of CH 4? 4) How many grams are there in 3.4 x molecules of NH 3? 5) How much does 4.2 moles of Ca(NO 3 ) 2 weigh? 6) What is the molar mass of MgO? 7) How are the terms molar mass and atomic mass different from one another? 8) Which is a better unit for expressing molar mass, amu or grams/mole?

21 Moles Worksheet (Solutions) 1) Define mole x of anything, usually atoms or molecules. 2) How many moles are present in 34 grams of Cu(OH) 2? 0.35 moles 3) How many moles are present in 2.45 x molecules of CH 4? 0.41 moles 4) How many grams are there in 3.4 x molecules of NH 3? 96 grams 5) How much does 4.2 moles of Ca(NO 3 ) 2 weigh? 689 grams 6) What is the molar mass of MgO? 40.3 grams/mole 7) How are the terms molar mass and atomic mass different from one another? Molar mass is used to describe the mass of one mole of a chemical compound, while atomic mass is used to describe the mass of one mole of an element or the mass of one atom of an element. 8) Which is a better unit for expressing molar mass, amu or grams/mole? Grams/mole is better, because any macroscopic amount of a substance is better expressed in grams than amu.

22 Name Period 7.1 THA MOLE! Worksheets 1. Find the molar mass of each compound. (Show your work!) a. Li2S b. FeCl3 c. Ca(OH)2 2. Define the following using your own words. a. atom: b. molecule: c. formula unit: 3. Label each of the following as atom, molecule, or formula unit. a. oxygen b. sodium sulfide 4. How many moles is each of the following? a X molecules NH3 c. sulfur dioxide d. potassium b. 1 billion (1 X 10 9 ) molecules O2 c X molecules Br2 5. Which contains more atoms? Justify your answer (hint remember definitions from your notes) 1.00 mol H2O2, 1.00 mol C2H6, or 1.00 mol CO? Find the mass of each substance: a mol C5H12 b mol F2 c mol H2O2 d mol NaOH

23 2. Calculate the volume of each of the following gases at STP: a. 7.9 mol Ar b mol O2 c mol C2H6 7.3 Write the 3 mole conversion factors: 1 mol = STP 1 mol = g 1 mol = particles 1. Calculate the percent composition of each compound: a. H2S b. (NH4)2C2O4 c. Mg(OH)2 2. Using your answers from #2, calculate the number of grams of these elements: a. sulfur in 7.23 g H2S b. nitrogen in 24.0 g (NH4)2C2O4 c. magnesium in 94.2 g Mg(OH)2 Empirical and Molecular Formulas Worksheet 1. The molecular formulas of some substances are as follows. Write their empirical formulas. a. Acetylene, C2H2 (used in oxyacetylene torches) b. Glucose, C6H12O6 (the chief sugar in blood) c. Octane, C8H18 (a component of gasoline) d. Ethylene glycol is C 2 H 6 O 2 (antifreeze)

24 2. Determine the empirical formula of a compound that contains 36.5% sodium, 25.4% sulfur, and 38.1% oxygen. 3. Nitrogen and oxygen form an extensive series of oxides with the general formula N x O y. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of this oxide? 4. An organic compound has an empirical formula of CH and a molecular mass of 78 g/mol. What is the molecular formula? 5. A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C 2 H 4 NO. If its molar mass is g/mol, what is the molecular formula of the compound? 6. Determine the molecular formula for each compound: (remember that you need to find empirical formula first!) a. 94.1% O and 5.9% H; molar mass = 34 g b. 40.0% C, 6.6% H, and 53.4% O; molar mass = 120 g

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