Practice Packet Unit 3: Moles & Stoichiometry - H. WONG
PRACTICE PACKET: Unit 3 Moles & StoichiometryRegents Chemistry: Mr. PalermoPractice Packet Unit 3:Moles & StoichiometryVocabulary:Lesson 1:Lesson 2:Lesson 3:Lesson 4:Lesson 5:Lesson 6:Lesson 7:Lesson 8:Lesson 9:www.mrpalermo.com1
PRACTICE PACKET: Unit 3 Moles & StoichiometryFor each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbookdefinitions. Write something to help you remember the word. Explain the word as if you were explainingit to an elementary school student. Give an example if you can. Don’t use the words given in yourdefinition!Mole:Molar Mass (gram formula mass):Reactants:Products:Coefficients (in reactions):Conservation of mass:Empirical Formula:Molecular Formula:Synthesis reaction:Decomposition reaction:Double replacement reaction:Single replacement reaction:Diatomic element:Polyatomic ion:Binary compound:Tertiary compound:Subscript:Superscript:Percent Composition:www.mrpalermo.com2
PRACTICE PACKET: Unit 3 Moles & StoichiometryLESSON 1: Moles and Molar MassObjective: Calculate Molar Mass (gram formula mass)1. Fill in the table belowFormulaa.HClO3b.Mg(OH)2Moles of eachatom1 mol of H atoms1 mol of Cl atoms3 mol of O atomsTotalmoles ofatoms5 mol ofatomsFormulac.CaCl2d.Mg3(PO4)2Moles of eachatomTotalmoles ofatomsCalculate the gram formula mass (molar mass) and don’t forget the units!!!1. CO26. H2SO42. FeS7. Al2(SO3)33. NaCl8. C12H22O44. Al2(CO3)39. Fe2O35. SiO2www.mrpalermo.com3
PRACTICE PACKET: Unit 3 Moles & Stoichiometry12. CH410. MgO13. NH311. Ca(OH)214. H2O2ASSESS YOURSELF ON THIS LESSON: /14If you missed more than 3, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 1:Find the gram formula mass of the following: (Show all work)1. MgO2. NaHCO33. C6H12O64. Al2O3ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /4If you missed more than 1 you should see me for extra help and/or re-watch the lesson video assignmentwww.mrpalermo.com4
Lesson 2: Calculating MolesObjective: Calculate the number of moles given the gramsCalculate the number of grams given the molesSolve for the mass given the moles. (Show your work)1.2.00 moles of C6H12O65.12.0 moles of SiO22.5.00 moles of SrSO46.0.330 moles of FeS3.0.250 moles of CH47.1.50 moles of MgO4.0.100 moles of NH38.0.500 moles of ZnCl25
Find the number of moles in the following measurements: (Show your work)9.900. grams C6H12O613.22 grams of CO210.24.5 grams H2SO414.20. grams of Fe2O311.192 grams SiO215.3.40 grams of H2O212.450. grams of ZnCl216.840. grams of NaHCO3ASSESS YOURSELF ON THIS LESSON: /14If you missed more than 3, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 21. What is the total number of moles in 80.0 grams of C2H5?2. How many grams are in 0.500 moles of CH4?3. How many grams are in 0.500 moles of ZnCl24. What is the total number of moles in 10. grams of Fe2O3?ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /4If you missed more than 1 you should see me for extra help and/or re-watch the lesson video assignment6
Lesson 3: Mole to Mole RatiosObjective: Calculate mole ratios in a chemical formulaUse the formula below to answer questions 1-73Cu 8HNO3 3Cu(NO3)2 2NO 4H2O1. If 1.00 mole of water is produced, how many moles of HNO3 are used?2. If 1.50 moles of copper are used, how many moles of NO are produced?3. If 4.50 moles of HNO3 are used, how many moles of copper (II) nitrate are produced?4. If 0.200 moles of NO are produced, how many moles of copper (II) nitrate produced?Use the formula below to answer questions 5-7Fe2O3 3CO 2Fe 2CO25. If 3.00 moles of Iron (III) oxide are used, how many moles of Iron are formed?6. If 2.50 moles of CO are used, how many moles of carbon dioxide are formed?7. If 8.56 moles of iron were produced, how many moles of the iron ore were used?7
Challenge Problems:Use the formula below to answer questions 8-103Cu 8HNO3 3Cu(NO3)2 2NO 4H2O8. If 9.00 grams of water are produced, how many moles of copper were used?9. If 3.00 moles of copper are mixed with 4 moles of HNO3, how many moles of NO can be formed?10. If 16.0 moles of HNO3 react with 4.00 moles of copper, how many moles of water are produced?ASSESS YOURSELF ON THIS LESSON: /10If you missed more than 2, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 3:1. Given the balanced equation: CaCO3(s) 2HCl(aq) CaCl2(aq) H2O(l) CO2(g) What is the totalnumber of moles of CO2 when 20. Moles of HCl is completely consumed?2. Given the balanced equation: F2(g) H2(g) 2HF(g) What is the total mole ratio of H2(g) to HF(g) inthe reaction?ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /2If you missed any problems you should see me for extra help and/or re-watch the lesson video assignment8
Lesson 4: Balancing ReactionsObjective: Assess and Balance chemical reactions using coefficients1. Which equation represents conservation of mass?(1) H2 Cl2 HCl(2) H2 Cl2 2HCl(3) H2 O2 H2O(4) H2 O2 2H2O2. A 4.86-gram sample of calcium reacted completely with oxygen to form 6.80 grams of calcium oxide.This reaction is represented by the balanced equation below. Determine the total mass of Oxygen thatreacted.2Ca(s) O2(g) 2CaO(s)BALANCE THE FOLLOWING REACTIONS18. Challenge:Fe2O3 CO Fe CO29
Regents Practice10
Types of ReactionsEquationReactant(s)Product(s)27.Cl2 2NaI 2NaCl I2Cl2 and NaINaCl and I228.HNO3 LiOH H2O LiNO329.2NaN3 2Na 3N230.Ba(NO3)2 K2SO4 2KNO3 BaSO431.BaO SO3 BaSO432.2Al Fe2O3 Al2O3 2Fe33.P4 6Cl2 4PCl334.2CH3OH(g) 3O2(g) 2CO2(g) 4H2O(g)Type ofReactionSinglereplacementAt your lab station, complete the following reactions below. Then determine what type of reactions is taking place.HCl(aq) Zn(s) ZnCl2(aq) H2(g)KI(aq) PB(NO3)2(aq) KNO3(aq) PbI2(aq)For each dark box define the word(s). Draw a particle diagram (model) to represent the phrase given. Then give achemical symbol as an example in that box.Synthesis reaction:Synthesis ReactionDecomposition ReactionSingle ReplacementDouble replacementDecomposition reaction:Single replacement reaction:Double replacement reaction:11
ASSESS YOURSELF ON THIS LESSON: /62If you missed more than 7, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 4Balance the following reactions and identify the type of reaction:1.NO O2 NO22.Ag S Ag2S3.Cu(OH)2 CuO H2O4.KClO3 KCl O25.Al O2 Al2O36.CO O2 CO2Draw a particle model to represent one physical change and 1 chemical change using real examples.ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /8If you missed more than 2 problems, you should see me for extra help and/or re-watch the lesson video assignment12
Lesson 5: Determining empirical and molecular formulasObjective: Determine the empirical formula from the molecular formulaDetermine the molecular formula from the empirical formulaBelow is a list of formulas. Write the empirical formula (if not already empirical)FormulaEmpiricalformula(simplest l2O2Empiricalformula(simplest ratio)Calculate the molecular formula from the empirical1. What is the molecular formula of a compound that has a mass of 276 and an empirical formula of NO2?2. What is the molecular formula of a compound that has a mass of 56g and an empirical formula ofCH2?3. What is the molecular formula of a compound that has a mass of 51g and an empirical formula ofHO?4. What is the molecular formula of a compound that has a mass of 289g and an empirical formula ofNH3?13
5. What is the molecular formula of a compound with a mass of 760g and an empirical formula ofCr2O3?C4H8O2C2H4O2ASSESS YOURSELF ON THIS LESSON: /26If you missed more than 4, do the Additional Practice. If not, go on to the next hw video!!!14
ADDITIONAL PRACTICE LESSON 51. What is the molecular formula of a compound that has a mass of 126g and an empirical formula ofSO2?2. What is the molecular formula of a compound that has a mass of 248g and an empirical formula ofNO3?3. Determine the empirical formula of C6H12O6ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /3If you missed any problems you should see me for extra help and/or re-watch the lesson video assignment15
Lesson 6: Percent CompositionObjective: Calculate Percent CompositionCalculate Percent composition of a hydrateDetermine the % composition of all elements in these compounds. Show all work!1) ammonium sulfiteFormula: (NH4)2SO3Mass of N%NMolar massMass of H%HMass of S%SMass of O%OFormula: Al(C2H3O2)3Mass of Al%AlMolar massMass of C%CMass of H%HMass of O%OFormula: NaBrMass of Na%NaMolar massMass of Br%Br2) aluminum acetate3) sodium bromidePercent Composition of a Hydrate4. Determine the percent by mass of water in the following hydrates.a.b. MgSO4 7H2O (GFM 246 g)Na2CO3 10H2O (GFM 286g)16
c.Initial mass of hydrate: 9.5 gFinal mass of anhydrous salt: 3.77 gd.Initial mass of hydrate: 5.3 gFinal mass of anhydrous salt: 4.1 g5. What is the percent composition of water in FeCl3 . 6H2O?ASSESS YOURSELF ON THIS LESSON: /5If you missed more than 1, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 61. copper (II) hydroxideFormula Cu(OH)2Mass of Cu%CuMolar massMass of O%OMass of H%HFormula: MgCO3Mass of Mg%MgMolar massMass of C%CMass of O%O2. magnesium carbonate3. If 125 grams of BaCl2 . 2H2O is completely dehydrated, how many grams of anhydrous BariumChloride will remain?ASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /3If you missed any problems you should see me for extra help and/or re-watch the lesson video assignment17
Lab Activity: Determining % Composition of a HydrateProcedure:1. Mass a crucible and cover.Mass of crucible and cover:2. Add approximately 1.9 grams of the unknown hydrate to the crucible and record the actual mass ofthe crucible, hydrate and cover. Place the crucible and contents with cover on the triangle with thecover off centered.Mass of crucible, cover, and Hydrate:3. Heat the crucible gently in the flame for 10 minutes.4. Let the crucible and cover cool for one minute. Then, using tongs mass the crucible, cover andcontents.Mass of crucible, cover, and product #1:5. Re-heat the sample for one minute, cool and re-mass. Repeat this step until the mass remainsconstant.Mass of crucible, cover, and product #2:Mass of crucible, cover, and product #3:Questions: SHOW ALL WORK1. Using YOUR DATA:a. Find the mass of the hydrateb. Find the mass of the anhydratec. Find the mass of water lost.d. Convert the mass of the anhydrate CuSO4 to moles.18
e. Convert the mass of water to moles.f. Divide the moles of water by the moles of anhydrate to find a whole number. This is thevalue of x in the formula CuSO4.xH2O.2. Calculate the percent of water in your hydrate.19
Lesson 7: Naming and Formula Writing for Binary CompoundsObjective: Identify binary compounds by name Construct chemical formulas for binary compoundsIonic Compounds require two types of ions: cations which are positive and anions which are negative. Allmetals (on the left side of the periodic table) form cations and nonmetals (on the left side of the periodictable) form anions primarily. In order to determine the formula of the compound they create you must makesure their ions sum to zero. For example, table salt is sodium chloride. Using the periodic table’s first set ofions, sodium forms 1 ions and chlorine forms -1 ions. Therefore their ions cancel out and the formula is NaCl. Itis not always that easy. Calcium chloride is the salt we put on roads to melt ice. Calcium forms 2 ions andChloride forms -1 ions. We need two chloride ions to balance the charges. The formula is CaCl2. Notice themetal, or positive cation is always written first! Try the following examples:1. Cesium fluoride:4. Barium sulfide:2. Potassium oxide:5. Aluminum chloride:3. Magnesium iodide:6. Calcium phosphide:There is a short cut called the drop and swap rule. Simply “drop” the charges from superscripts to subscriptsand switch their order. In example 6 above, calcium phosphide had charges 2 and -3 respectively. Drop thecharges to form uncharged subscripts 2 and 3 and reverse to form Ca3P2.Try the drop and swap rule to find the formula and don’t forget to reduce if uminumAlCl3MagnesiumZinc20
Now we know how to write formulas from their names but we also need to know how to write names fromformulas. The rule is: write the whole name of the first element and the second element drop the ending andreplace with “ide.” For example: H2S is hydrogen sulfide. In this case, the amount of each element doesn’taffect the name of the compound. Use table S to help you find names. Try to name the following examples:1. NaF6. NaH2. MgCl27. K3P3. Al2O38. MgO4. MgI29. Li2Te5. H2O10. AlCl3ASSESS YOURSELF ON THIS LESSON: /35If you missed more than 5, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 7Write the name of the following:Write the chemical formula for the following:1. CaCl24. zinc oxide2. NaBr5. potassium bromide3. NaS6. Aluminum nitrideASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /6If you missed more than 1 problem you should see me for extra help and/or re-watch the lesson video assignment21
Lesson 8: Naming and Formula Writing with Multiple Oxidation StatesObjective: Identify binary compounds containing multiple charges by name using roman numerals Construct chemical formulas for binary compounds containing multiple chargesIf the first substance in a compound has more than 1 oxidation state you must write the charge used (romannumerals in parenthesis).Transition metals refer to the metals in groups 3-12 of the period table(elements Sc through Zn and down). These metals form various positiveions and therefore have more than one oxidation state (charge). It isimportant to identify which ion is used when naming the compound.We will work backwards to do this, meaning, we will look at the chargefor the second ion in the formula to find that charge of the first. We willreport the charge of the first ion in roman numerals (the numerals youneed to memorize are listed to the right) in parenthesis after that ion.For example:OneIFiveVTwo IISixVIThree IIISeven VIIFour IVCuOO is -2 so Cu needs to be 2Copper (II) oxideCu2OO is -2 so each Cu must be 1Copper (I) oxideThese two compounds have different structures and properties and must have different names. Try to namethe following compounds with transition metals:1. FeBr26. NiF32. FeBr37. CuCl3. PbS8. CuCl24. PbS29. CuS5. NiO10. Cu2S22
Formula writing may seem easier. You can still use the drop and swap rule. Remember the number in romannumerals refers to the charge of the first ion. Try to give the formula of the following compounds:1. Chromium (VI) oxide6. Zinc (II) oxide2. Manganese (VII) chloride7. Iron (II) oxide3. Lead (IV) iodide8. Iron (III) oxide4. Silver (I) sulfide9. Gold (III) phosphide5. Nickel (II) fluoride10. Titanium (IV) sulfideASSESS YOURSELF ON THIS LESSON: /35If you missed more than 5, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 8Write the name of the following:Write the chemical formula for the following:1. FeCl 24. copper (I) bromide2. FeCl 35. copper (II) bromide3. Ag3N6. Aluminum bromideASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /3If you missed any problems you should see me for extra help and/or re-watch the lesson video assignment23
Lesson 9: Naming and Formula Writing Tertiary CompoundsObjective: Identify tertiary compounds containing polyatomic ions by name Construct chemical formulas for tertiary compounds containing polyatomic ionsBinary compounds have only two elements in their formula, as we saw in exercises above. Tertiarycompounds have three or more elements in their formula and have a new system of naming. Thesecompounds have a polyatomic ion, which is an ion that has a few elements grouped together with only onecharge between them. A common example is OH- which shows two elements with an overall charge of -1. Asbefore, name the first element completely and then look up the rest of the compound on table E of thereference tables. Make sure you copy the right one, some are very similar! For example: NaOH is calledsodium hydroxide. Also, beware of NH4 which is the only polyatomic cation (that comes in front). Try namingthe following examples:1. KHCO34. LiNO22. CaSO45. Cu(ClO4)23. NaNO36. Al2(SO3)3To write the formula of a tertiary compound you can still use the drop and swap rule, however, you must besure to only drop the superscripts and leave the subscripts alone. For example, aluminum carbonate:Al 3 and CO3-2Leave the 3 alone! Swap the 3 and 2Al2(CO3)3Remember, formulas don’t show any charges. You can see that we use parenthesis around the polyatomic ionbecause the entire ion charge was -2 and must swap with aluminum so the entire ion gets aluminum’s 3. Tryto write the formula for the following compounds (write the formulas of the ions next to the name diumCalciumAmmoniumIron (II)Aluminum24
1. Zinc Hydroxide:4. Magnesium oxalate:2. Calcium chlorate:5. Lead (IV) chromate:3. Hydrogen acetate:6. Strontium cyanide:ASSESS YOURSELF ON THIS LESSON: /37If you missed more than 6, do the Additional Practice. If not, go on to the next hw video!!!ADDITIONAL PRACTICE LESSON 9Write the name of the following:Write the chemical formula for the following:1. KNO34. aluminum phosphate2. LiOH5. strontium acetate3. Ni(OH)26. Aluminum sulfateASSESS YOURSELF ON THIS ADDITIONAL PRACTICE: /6If you missed any problems, you should see me for extra help and/or re-watch the lesson video assignment25
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PRACTICE PACKET: Unit 3 Moles & Stoichiometry 3 www.mrpalermo.com Objective: Calculate Molar Mass (gram formula mass) LESSON 1: Moles and Molar Mass 1. Fill in the table below Formula Moles of each atom Total moles of atoms Formula Moles of each atom Total moles of atoms a. HClO 3 1 mol of H atoms 1 mol of Cl atoms 3 mol of O atoms 5 mol of
13 Molarity Moles of solute/Liters of Solution (M) Molality Moles of solute/Kg of Solvent (m) Mole Fraction Moles solute/total number of moles Mass % Mass solute/total mass x 100 Volume % volume solute/total volume x 100 ppm parts per million * ppb parts per billion * Chemical concentrations * mass for solutions, volume for gasses Molarity Moles of solute/Liters of Solution (M)
point at which an indicator changes color is called the end point of the titration. Phenolphthalein is an appropriate choice for this titration. In acidic solution, phenolphthalein is colorless, and in basic solution, it is pink. At the equivalence point, the number of moles of acid equals the number of moles of base. (1) moles of H 3O moles of OH
NEET (UG)-2019 (Code- 1)Q 6. The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber's process is : (1) 20 (2) 30 (3) 40 (4) 10 Answer (2) Sol. Haber's process N22 3(g) 3H (g) 2NH (g) 20 moles need to be produced 2 moles of NH 3 3 mol
Total nurnber of moles of solution before adsorption, moles Change in mole fraction of surfactant resulting from adsorption Mass of insoluble adsorbent, kg Amount adsorbed, mol rnS2 Number of moles of surfactant adsorbed. moles Surface area of substrate, m' Zeta potential, V Fluid density, kg m" Particle density, kg m-' Fluid viscosity. N s rn"
PRACTICE PACKET: Unit 7 Moles & Stoichiometry 5 www.chempride.weebly.com ADDITIONAL PRACTICE LESSON 1: Find the gram formula mass of the following: (Show all work) 1. MgO 5. Ca(OH) 2 2. NaHCO 3 6. CH 4 3. C 6 H 12 O 6 7. NH 3 4. Al
Acme Packet 1100 Acme Packet 3900 Acme Packet 4600 front bezel hides the fan assemblies without restricting airflow through the system. Acme Acme Packet 6100 Acme Packet 6300 Packet 6300 Acme Packet 6350 The rear of Acme Packet 6300 least one slot reserved for an NIU.
Practice Packet: Unit 9 - Moles/Stoichiometry 1 LESSON 10.1: Solubility Curves and Table G Objective: Calculate Molar Mass (gram formula mass) 1. Use the graph to the right to find the mass of solute that will dissolve in 100 mL of water at the following temperatures to make saturated solutions. a. KNO 3 at 70 C _ b.
Plan and monitor animal diet and nutrition LANAnC46 Plan and monitor animal diet and nutrition 1 Overview This standard covers planning and monitoring the diet and nutrition for animals in your care. You will need to identify the nutritional requirements of the animals and develop feeding plans containing all the necessary information for those responsible for feeding the animals. You will .
