ࡱ>  68 /012345fh bjbj M*%KKK4h%9+O+O+O+r@j@,AaccccccfRcK A2@@r@ A AcO+O+xdOdOdO A2O+KO+adO AadOdOaIєO+ pfD~FM0+ZVLZєєZKh A AdO A A A A AccMx A A A A A A AZ A A A A A A A A A : WPHS Chemistry Unit 5 Packet Stoichiometry  INCLUDEPICTURE "http://www.beaconhurst.stirling.sch.uk/departments/science/chem7.jpg" \* MERGEFORMATINET  Bergmann-Sams Chemistry: Unit 5 Outline: Stoichiometry AssignmentMust be done in classPodcast 5.1Worksheet 5.1Lab: Simple Weight Loss Podcast 5.2 (OPTIONAL/AS NEEDED)Worksheet 5.2Podcast 5.3Worksheet 5.3Lab: VinegarNaHCO3Podcast 5.4Worksheet 5.4Lab: Limiting Reactant Exploration LabLab: Limiting Reactant LabPodcast 5.5Worksheet 5.5Take Home Lab (Cookies-Optional)Unit 5 ReviewsheetUnit 5 VocabularyLab ExamUnit 5 Exam Unit 5: Vocabulary Stoichiometry Limiting reagent/limiting reactant Excess reagent/excess reactant Theoretical yield Actual yield Percent yield  SHAPE \* MERGEFORMAT  (OPTIONAL) Take Home Lab: Making Chocolate Chip Cookies Name The following recipe for chocolate chip cookies recently appeared in Chemical & Engineering News (C&EN, Jun 19, 1995, p. 100). It was attributed to Jeannene Ackerman of Witco Corp. Ingredients: 1587.5 cm3 gluten24.9 cm3 NaHCO334.9 cm3 refined halite4176.25 cm3 partially hydrogenated tallow triglyceride5177.45 cm3 crystalline C12H22O116177.45 cm3 unrefined C12H22O1174.9 cm3 methyl ether of protocatechuic aldehyde8Two calcium carbonate-encapsulated avian albumen-coated protein9473.2 cm3 theobroma cacao10236.6 cm3 de-encapsulated legume meats (sieve size #10) To a 2-L jacketed round reactor vessel (reactor #1) with an overall heat-transfer coefficient of about 100 Btu/F-ft2-hr add one, two, and three with constant agitation. In a second 2-L reactor vessel with a radial flow impeller operating at 100 rpm add four, five, six, and seven until the mixture is homogeneous. To reactor #2 add eight followed by three equal portions of the homogeneous mixture in reactor #1. Additionally, add nine and ten slowly with constant agitation. Care must be taken at this point in the reaction to control any temperature rise that may be the result of an exothermic reaction. Using a screw extrude attached to a #4 nodulizer place the mixture piece-meal on a 316SS sheet (300 x 600 mm). Heat in a 460K oven for a period of time that is in agreement with Frank & Johnston's first order rate expression (see JACOS, 21, 55), or until golden brown. Once the reaction is complete, place the sheet on a 25C heat-transfer table allowing the product to come to equilibrium. Conversion Factors 1 teaspoon = 5cm3 235 cm3 = 1 cup C = 9/5F +32 To Receive Credit: You must have a signed note from your parent/guardian that indicates that you made the cookies you can even bring in a sample to your friendly Chemistry Teacher. PROBLEMS: Use dimensional analysis to set up the problem. Please show your work! Show your work here for how much of each item you need to measure out at home: How many cookies did you made from this recipe? If you only have 100cm3 of unrefined C12H22O11, how much gluten will you need? You have decided with a group of friends to make these cookies for a fund raiser. It is your job to make 1000 cookies. How many calcium carbonate-encapsulated avian albumen-coated protein will you need to buy? Adjust the recipe for 3 calcium carbonate-encapsulated avian albumen-coated protein and determine how much of each reactant you need in the recipe. STOICHIOMETRY LABSimple Weight Loss A balanced equation indicates the proportions between reactants and products. More specifically, the coefficients in the equation indicate the mole ratios between the chemical substances. Thus, it is possible to determine how much product will be produced from a given amount of reactant. This predicted amount can then be compared with the actual amount produced to determine the percent yield of the reaction. In this experiment, you will investigate two reactions: Copper and aqueous silver nitrate yield silver and aqueous copper(II) nitrate. Sodium bicarbonate and aqueous sulfuric acid produce aqueous sodium sulfate, water, and carbon dioxide gas. SAFETY 2M sulfuric acid can cause burns. Avoid skin and eye contact. Rinse spills with plenty of water. PROCEDURE Obtain a beral pipet containing 2M H2SO4. Obtain a clean, dry flask. Measure and record its mass. Place approximately 0.30g of NaHCO3 into the flask. Find the combined mass of the flask and sodium bicarbonate and record. Determine the exact mass of sodium bicarbonate by subtraction. This mass must be between 0.20 and 0.40 g. Record the mass of sodium bicarbonate in a data table. Record the TOTAL mass of all the components of the lab: sodium bicarbonate, flask, dropper and sulfuric acid. SLOWLY, drop by drop, add the sulfuric acid to the sodium bicarbonate to generate carbon dioxide gas. Continue releasing the acid in this manner until gas production ceases. Measure and record the TOTAL mass of all the components again (like in step 4). Return the beral pipet with the remainder of the sulfuric acid. Rinse the contents of the flask down the drain with water. Clean up your lab station. DATA Construct a data table for each reaction to display your laboratory measurements. Make sure that each value is clearly labeled. ANALYSIS Write a balanced equation for the reaction. Calculate the actual mass of carbon dioxide produced (actual yield). Using the balanced equation, calculate the mass of carbon dioxide that should be produced from the mass of sodium bicarbonate that you used (theoretical yield). CONCLUSIONS Calculate the percent yield of the carbon dioxide using the equation below (show your work). % yield =experimental yield( 100theoretical yield A perfect percent yield would be 100%. Comment on your degree of accuracy and suggest possible sources of measurement error. How could these errors be reduced in the future? Limiting Reactant Exploration Lab: How much Carbon Dioxide? Introduction: In this lab you will do a cool reaction, make some measurements, make a graph, and then write down some observations. The reaction that you will do is the reaction between vinegar and baking soda. In this reaction, carbon dioxide, CO2 will be produced. Chemists use chemical symbols to show the reaction. The reaction is: CH3COOH (aq)+NaHCO3(H2O+CO2+NaCH3COOVinegarBaking SodaWaterCarbon DioxideSodium Acetate Materials: Apparatus as pictured below Vinegar Baking Soda To simplify: Here is a picture of what you will need:  INCLUDEPICTURE "http://www.pasco.com/experiments/chemistry/april_2003/photos/balance.jpg" \* MERGEFORMAT  Procedure: Follow this procedure as closely as possible. place 0.25 g into a paper towel Get the appropriate amount of vinegar into the flask Set-up the apparatusand mix. Record the amount of CO2 collected Data Fill out the following data table: Amount of vinegarAmount of baking sodaVol CO211 mL0.25g 22 mL0.25g 33 mL0.25g 44 mL0.25g 55 mL0.25g 66 mL0.25g  HAVE YOUR TEACHER SIGN HERE IMMEDIATELY AFTER COLLECTING DATA Questions Describe in detail what occurred (your observations) when the vinegar was mixed with the baking soda. Some descriptive words that you should probably use are, but not including (gas given off, fizzing, foaming, balloon expanding) Describe the pattern of how much carbon dioxide, CO2 was formed as you added more and more vinegar. Relate this to the graph. For each trial: explain which substance was the limiting and excess reagent. Explain how you were able to determine this. You should have noticed that as you increased the amount of vinegar eventually you got the same amount of carbon dioxide, CO2. Explain why that occurred.  Chemistry Limiting Reactant Lab Introduction A limiting reactants is defined as one of the reactants in a chemical reaction that will be used up first. The purpose of this lab is to determine the amount of precipitate that will be produced when a given amount of calcium chloride and sodium sulfate are mixed. Once you have massed the calcium chloride and the sodium sulfate you will need to do each of the following before you proceed with the rest of the experiment. Write the balanced chemical reaction noting the states of matter for all substances. (See solubility chart to determine which substance precipitates.) Determine which reagent, calcium chloride or sodium sulfate, is limiting. Predict the amount of the precipitate that will be produced. Once you have done these three things, show them to your instructor. Then you may begin the experiment. Procedure Label and mass a test tube. The test tube must be completely dry Obtain about 0.30 grams of each reagent (It doesnt matter how much you get just as long as you know exactly how much you obtain), and determine both which reagent is limiting and how much precipitate you will discover. Dissolve the calcium chloride into 3 mL of deionized water by carefull flicking the test tube (Your instructor will show you how to do this. Dissolve the sodium sulfate into 3-mL of deionized water. Pour the sodium sulfate solution into the test tube with calcium chloride in it. Take care to get all of the sodium sulfate into the calcium chloride test tube. Remove the stopper and then place your sample into a centrifuge and spin out the precipitate. (Caution should be used in using this device. Your teacher will instruct you on proper use of a centrifuge) Decant, or pour off, the liquid (supernatant) above the precipitate. Be careful not to allow any of the precipitate to be poured out. Add about 10-mL of deionized water to your precipitate and spin it again. Decant again and repeat this step two more times for a total of four centrifuges SHOW YOUR PRODUCT TO YOUR TEACHER AND GET HIS SIGNATURE. Set your labeled test tube into a drying oven overnight. Weigh your test tube and determine the mass of the precipitate that you have. SHOW YOUR PRODUCT TO YOUR TEACHER AND GET HIS SIGNATURE AGAIN. Compare this amount to what you expected to get from your calculations. Calculations Show all calculations needed to determine the expected amount of precipitate required to do the experiment. This should include the balanced chemical reaction and all appropriate stoichiometric calculations. Questions Why did you have to mass the test tube prior to beginning the experiment? Why did you need to add water to the solid calcium chloride and solid sodium sulfate to cause the reaction to occur? Comment on sources of error. What was your percentage of error? Draw a picture of the two test tubes prior to adding the two chemicals. What had happened to the calcium chloride? What happened to the sodium sulfate. Now draw a picture of the test tube once you have mixed the two chemicals. Where are all of the chemicals now? Label this in your diagram. Worksheet 5.1 Stoichiometry 1. Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide: 5C(s) + 2SO2(g) -----> CS2(s) + 4CO(g) a. How many moles of CS2 form when 6.3 mol of C reacts? How many moles of carbon are needed to react with 7.24 moles of SO2 Silver can be made according to the following equation: ___AgNO3+ ___Ca ( ___Ca(NO3)2 + ___Ag Balance the equation If 35.3 moles of silver nitrate are reacted how many moles of silver are produced? Barium oxide reacts with carbon dioxide to make Barium carbonate: ___BaO + ___CO2 ( ___BaCO3 Balance the equation If 23.4 moles of barium oxide react, how many liters of CO2 are required at STP? Car batteries are called lead storage batteries because of their use of large quantities of lead. These batteries utilize the following equation. Pb + PbO2 +2H+ + 2HSO4- ( 2PbSO4 + 2 H2O If 34.3-g of PbO2 react how many grams of water will be formed? Assuming the same mass of PbO2, how many grams of PbSO4 will be formed? Ammonia, (NH3) is produced by reacting its elements with each other according to the following equation: ___N2 + ___H2 ( ___NH3 Balance the equation. If 34.3-L of nitrogen is reacted with hydrogen, how many liters at STP of ammonia will be formed? 6. 32.5-g of ZnSO4 reacts to form how many grams of BaSO4 according to the following equation. Dont forget to balance the equation. ___ZnSO4 + ___BaCl2 ( ___BaSO4 + ___ZnCl2 7. When sodium metal is added to water the resulting gas, Hydrogen can often explode. How many Liters of hydrogen gas is produced when 41.2-g of sodium is dropped into water. Again, you must balance the equation in order to solve the problem. ___Na + ___HOH ( ___NaOH + ___H2 8. Propane is a gas used often for backyard grills. How many Liters of CO2 is produced when 54.9-L of propane (C3H8) is burned according to the following equation. Again, you must balance the equation in order to solve the problem. ___C3H8 + ___O2 ( ___CO2 + ___H2O Worksheet 5.2 More Stoichiometry How many moles of Carbon dioxide is formed when 44-mol of CH4 is burned? 43.5-grams of barium sulfate is formed from the reaction of barium nitrate and sodium sulfate. How many moles of sodium sulfate reacted? 32.3-L of O2 is formed when KClO3 is decomposed. How many moles of KClO3 reacted initially? __KClO3 ( __KCl + __O2 22.8-g of NaOH is reacted with hydrochloric acid. How many grams of water is formed? 32.5-grams of iron III chloride reacts with silver nitrate. How many grams of silver chloride are formed? 43.5-grams of copper II sulfate is reacted with barium nitrate. How many grams of precipitate are formed? How many liters of hydrogen gas is formed when 13.5-grams of calcium reacts with sulfuric acid (H2SO4)? Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride. A volume of 7.5 L of hydrogen gas was produced from the single replacement reaction of zinc and nitric acid (HNO3). Calculate the mass of zinc needed for this reaction. How many molecules of chlorine are needed to react with 5.6 g of iron to form iron III chloride? Worksheet 5.3 Limiting Reactants BOX ALL ANSWERS!! 1. When 114.0 g of iron and 292.7 g of chlorine gas reacts, iron(III) chloride is formed. a. Write a balanced equation b. How many grams of Iron (III) chloride is formed c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? 2. 20 L of oxygen react with 1.0L of methyl alcohol, CH3OH a. Write a balanced equation b How many liters of water will be formed at STP? c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? 3. 25 g of hydrazine, N2H4(l), and 66 g of hydrogen peroxide, H2O2(l), react to produce nitrogen gas and water. a. Write a balanced equation b. How many grams of nitrogen are produced? c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? 4. 22.5 grams of lithium reacts with 33.5 grams of aqueous aluminum sulfate. This is a single replacement reaction. a. Write a balanced equation. b. How many grams of lithium sulfate will be formed? c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? 5. 33.6 grams of sulfur dioxide reacts with 55.3 grams of water to form sulfurous acid (H2SO3). a. Write a balanced equation. b. How many grams of sulfurous acid will be formed? c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? 6. 77 g of potassium iodide react with 32 g of lead II nitrate reacts to form a yellow precipitate. a. Write a balanced equation and identify the precipitate b. How many grams of the precipitate will be formed? c. What is the limiting reactant? d. How much excess reagent is left over at the end of the experiment? Worksheet 5.4 Percent Yield 1. 15.5-g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.5-g AgCl is produced. NH4NO3 is the other product. What is the percent yield?  EMBED Equation.3  2. Potassium Chlorate decomposes according to the following reaction. 2KClO3 ( 2KCl +3O2 In an experiment 32.5-g of KClO3 is decomposed and 15.2-g of KCl is formed. What is the percent yield? 3. Nitrogen gas reacts with hydrogen gas to make ammonia (NH3). 15.5-L of N2 reacts at STP to make 30-L of ammonia. What is the percent yield? What is the percent yield of oxygen gas if 54L of O2 can be obtained from the thermal decomposition of 500.0 g of potassium chlorate? KClO3 ( KCl + O2 5. It is desired to prepare 100.0g of silicon tetrafluoride by adding hydrogen fluoride to silicon dioxide. The percent yield of this process is 75%. Ho much HF do you need to react? The other product is water. 6. When black gunpowder explodes, potassium nitrate, carbon, and sulfur react with each other to form nitrogen gas, carbon dioxide gas, and solid potassium sulfide. If the original mixture contains 50.0 g of potassium nitrate, if the total volume of the gases is 20L, then what is the percent yield for this process? 7. Very hot zinc will react with steam to form zinc oxide and hydrogen. 5.4L of H2 was used to use up 20.0 g of zinc completely? What is the percent yield of this process? Worksheet 5.5 Molar Mass Worksheet Name _________________ 2.35g of metal with a charge of +2 reacts with hydrochloric acid to produce 0.598 L of gas at STP. What metal do you have? M + HCl ( MCl2 + H2 (NH4)3PO4 reacts with 0.0345 g of metal sulfate (M2(SO4)3) to produce 0.0399 g of (NH4)2SO4. Balance the equation. What is the molar mass of the metal? What is the metal? __M2(SO4)3 + __(NH4)3PO4 ( __(NH4)2SO4 + __MPO4 3.45g of a metal hydroxide with charge + 1 reacts with excess Iron III Chloride to make 0.82g of Iron III hydroxide. What is the identity of the metal hydroxide? 30.2 L of oxygen is produced at STP when 135.9 g of metal chlorate of charge +3 decomposes into oxygen and the metal chloride. What is the identity of the metal chlorate? Unit 5 Reviewsheet 1. How many grams of water are formed when 12.5-g of hydrogen reacts with oxygen? 2. How many liters of carbon dioxide are formed when 12.3-g of sodium carbonate reacts with 2.0-L of hydrogen chloride. The reaction is printed below: ___Na2CO3 + ___HCl ( ___NaCl + ___H2O + ___CO2 3. How many grams of precipitate are formed when 24.3-g of zinc nitrate reacts with 20.5-g of sodium phosphate? 4. How many liters of oxygen are produced when 3.25-g of KClO3 decomposes into KCl and O2? 5. When 2.25-g of sodium chloride reacts with excess silver nitrate, 3.45-g of precipitate is formed. What is the percent yield of the precipitate? 6. 4.35-g of C5H12 reacts with 4.0-L of O2. a. How many liters of CO2 are formed? b. How much excess reactant remains? 7. 3.0-g of zinc reacts with silver nitrate to form how many grams of zinc nitrate? 8. 8.2-mol of barium carbonate decomposes into how many moles of barium oxide. The other product is carbon dioxide. 9. 4.5-g of sodium hydroxide reacts with 2.0-g of sulfuric acid (H2SO4). How many grams of water are formed? 10. 8.0-L of butane (C4H10) reacts with oxygen to make 50-g of carbon dioxide. What is the percent yield? 11. 8.5-L of hydrogen reacts with 5.4-L of nitrogen to make a. how many liters of ammonia (NH3)? b. How many liters of excess reactant remains? 12.A 2.25-g sample of aluminum sulfate reacts with 3.25-g of sodium phosphate to make 1.0-g of precipitate. What is the percent yield? Stoichiometry Worksheet 1 KEY 1. Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide: 5C(s) + 2SO2(g) -----> CS2(s) + 4CO(g) How many moles of CS2 form when 6.3 mol of C reacts? How many moles of carbon are needed to react with 7.24 moles of SO2  EMBED Equation.3  2. Silver can be made according to the following equation: 2AgNO3+ Ca( Ca(NO3)2 + 2Ag 35.3g ?g Balance the equation If 35.3 moles of silver nitrate are reacted how many moles of silver are produced?  EMBED Equation.3  3. Barium oxide reacts with carbon dioxide to make Barium carbonate: BaO + CO2 -( BaCO3 (Balanced) 23.4mol L? Balance the equation If 23.4 moles of barium oxide react, how many liters of CO2 are required at STP?  EMBED Equation.3  4. Car batteries are called lead storage batteries because of their use of large quantities of lead. These batteries utilize the following equation. Pb + PbO2 +2H+ + 2HSO4- (2PbSO4 + 2 H2O 34.3g g? If 34.3-g of PbO2 react how many grams of water will be formed? Assuming the same mass of PbO2, how many grams of PbSO4 will be formed?  EMBED Equation.3  5. Ammonia, (NH3) is produced by reacting its elements with each other according to the following equation: N2 + 3H2 ( 2NH3 34.3L L? Balance the equation. If 34.3-L of nitrogen is reacted with hydrogen, how many liters at STP of ammonia will be formed?  EMBED Equation.3  6. 32.5-g of ZnSO4 reacts to form how many grams of BaSO4 according to the following equation. Dont forget to balance the equation. ZnSO4 + BaCl2 ( BaSO4 + ZnCl2 bal 32.5g g?  EMBED Equation.3  7. When sodium metal is added to water the resulting gas, Hydrogen can often explode. How many Liters of hydrogen gas is produced when 41.2-g of sodium is dropped into water. Again, you must balance the equation in order to solve the problem. 2Na + 2HOH ( 2NaOH + H2 41.2g L?  EMBED Equation.3  8. Propane is a gas used often for backyard grills. How many Liters of CO2 is produced when 54.9-L of propane (C3H8) is burned according to the following equation. Again, you must balance the equation in order to solve the problem. C3H8 + 5O2 ( 3CO2 + 4H2O 54.9L L?  EMBED Equation.3  Stoichiometry WS B Name Period 1. How many moles of Carbon dioxide is formed when 44-mol of CH4 is burned?  EMBED Equation.3 +4 2. How many moles of calcium phosphate is formed when 32.5-mols of calcium nitrate reacts with sodium phosphate?  EMBED Equation.3  3. 43.5-grams of barium sulfate is formed from the reaction of barium nitrate and sodium sulfate. How many moles of sodium sulfate reacted?  EMBED Equation.3  4. 32.3-L of O2 is formed when KClO3 is decomposed. How many moles of KClO3 reacted initially?  EMBED Equation.3  5. 2.5-mol of water is made from its elements. How many particles of hydrogen reacted?  EMBED Equation.3  6. 22.8-g of NaOH is reacted with hydrochloric acid. How many grams of water is formed?  EMBED Equation.3  7. 32.5-grams of iron III chloride reacts with silver nitrate. How many grams of silver chloride are formed?  EMBED Equation.3  8. 34.5-grams of Lithium reacts with Chromium III chloride. How many grams of lithium chloride is formed?  EMBED Equation.3  9. 43.5-grams of copper II sulfate is reacted with barium nitrate. How many grams of precipitate are formed?  EMBED Equation.3  10 How many liters of hydrogen gas is formed when 13.5-grams of calcium reacts with sulfuric acid?  EMBED Equation.3  11. 45.6-L of H2 is formed when zinc is reacted with nitric acid. How many grams of zinc reacted?  EMBED Equation.3  12. 14.5-g of cesium explosively reacts with water to form hydrogen and cesium hydroxide. How many molecules of hydrogen were formed?  EMBED Equation.3  13. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride. 2Ag+Cl2(2AgCl?84g  EMBED Equation.3  14. A volume of 7.5 L of hydrogen gas was produced from the single replacement reaction of zinc and nitric acid (HNO3). Calculate the mass of zinc needed for this reaction. Zn+2HCl(ZnCl2+H2g?7.5L EMBED Equation.3  15. How many molecules of chlorine are needed to react with 5.6 g of iron to form iron III chloride? 3Cl2+2Fe(2FeCl3Molec?5.6g EMBED Equation.3  16. What mass of ammonia, NH3, is necessary to react with 2.1 x 1024 molecules of oxygen when ammonia (NH3) reacts with oxygen to form water and nitrogen dioxide? 4NH3 +7O2(4NO2 + 6H2Og?2.1 x 1024 molec EMBED Equation.3  17. Calculate the volume of carbon dioxide produced when 250 g of pentane, C5H12, burn. Assume the carbon dioxide is cooled to STP. C5H12+8O2(5CO2+6H2O250g?L EMBED Equation.3  18. Nitrogen gas reacts with oxygen to form dinitrogen trioxide. How many molecules of oxygen are needed to make 5.5 L of N2O3 at STP? 2N2+3O2(2N2O3molec?5.5L EMBED Equation.3  19. Silver Nitrate reacts with sodium chloride to make the silver chloride and sodium nitrate. When 2.53 grams of silver nitrate is reacted. How many grams of silver chloride are formed? AgNO3+NaCl(AgCl+NaNO32.53g?g EMBED Equation.3  20. Methane (CH4) is burned in air. When 50.6 L of methane is burned how many grams of carbon dioxide will be formed? CH4+2O2(CO2+2H2O50.6L?g EMBED Equation.3  21. Calcium Carbonate decomposes into calcium oxide and a common gas. When 45.5 grams of calcium oxide is formed how many liters of gas is also formed from this reaction. CaCO3(CaO+CO245.5g?L  EMBED Equation.3  22. When 3.25 g of copper II nitrate reacts with ammonium hydroxide. How many grams of the precipitate will form. Cu(NO3)2+2NH4OH(Cu(OH)2 (s)+2NH4NO3 (aq)3.25g?g=ppt EMBED Equation.3  +88 Limiting Reactant Worksheet Do all work on a separate sheet of paper and BOX ALL ANSWERS!! 1. When 114.0 g of iron and 292.7 g of chlorine gas reacts, iron(III) chloride is formed. a. Write a balanced equation b. What is the limiting reactant? c. How many grams of Iron (III) chloride is formed How much excess reagent is left over at the end of the experiment?  EMBED Equation.3  2. 20 L of oxygen react with 1.0L of methyl alcohol, CH3OH a. Write a balanced equation b. What is the limiting reactant? c How many liters of water will be formed at STP? d. How much excess reagent will be left over?  EMBED Equation.3  3. 25 g of hydrazine, N2H4(l) and 66 g of hydrogen peroxide, H2O2 (l) react exothermically to produce nitrogen gas and water. a. Write a balanced equation b. What is the limiting reactant? c. How many grams of nitrogen are produced? d. How much excess reagent is left over?  EMBED Equation.3  4. 22.5 grams of lithium reacts with a 33.5 grams of aqueous aluminum sulfate according to a single replacement reaction. a. Write a balanced equation. b. What is the limiting reactant? c. How many grams of lithium sulfate will be formed? d. How much excess reagent will remain?  EMBED Equation.3  5. 33.6 grams of sulfur dioxide reacts with 55.3 grams of water to form sulfurous acid. a. Write a balanced equation. b. What is the limiting reactant? c. How many grams of sulfurous acid will be formed? d. How much excess reagent will remain?  EMBED Equation.3  6. 77 g of potassium iodide react with 32 g of Lead II nitrate reacts to form a yellow precipitate. a. Write a balanced equation and identify the precipitate b. What is the limiting reactant? c. How many grams of the precipitate will be formed? d. How much excess reagent will remain?  EMBED Equation.3  *7. In the following equation: NH3 + O2 ---> H2O + NO2, a. Balance the equation b. What is the limiting reactant? c. If you react 22 L of NH3 with 95 L of air (Which is 20% oxygen), how many liters of NO2, will be produced? d. How much excess reagent will remain?  EMBED Equation.3  WS D: Percent Yield Worksheet 1. 15.5-g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.5-g AgCl is produced. NH4NO3 is the other product. What is the percent yield? NH4Cl+AgNO3(AgCl+NH4NO315.5g35.5g EMBED Equation.3   EMBED Equation.3  2. Potassium Chlorate decomposes according to the following reaction. 2KClO3 ( 2KCl +3 O2 In an experiment 32.5-g of KClO3 is decomposed and 15.2-g of KCl is formed. What is the percent yield? 2KClO3(2KCl+3O232.5g15.2g EMBED Equation.3  3. Nitrogen gas reacts with hydrogen gas to make ammonia (NH3). 15.5-L of N2 reacts at STP to make 30-L of ammonia. What is the percent yield? N2+3H2(2NH315.5L30L EMBED Equation.3  4. The Haber and Caude processes are methods by which ammonia (NH3) is synthesized from its elements (H2 and N2) What is the percent yield if 5.0-kg of ammonia (in Kilograms) is to be expected when 4000.0 L of nitrogen are used in these procedures?  EMBED Equation.3  5. What is the percent yield of oxygen gas if 54L of O2 can be obtained from the thermal decomposition of 500.0 g of potassium chlorate?  EMBED Equation.3  6. It is desired to prepare 100.0g of silicon tetrafluoride by adding hydrogen fluoride to silicon dioxide. The percent yield of this process is 75%. Ho much HF do you need to react?  EMBED Equation.3  7. When black gunpowder explodes, potassium nitrate, carbon, and sulfur react with each other to form nitrogen, carbon dioxide, and potassium sulfide. If the original mixture contains 50.0 g of potassium nitrate, if the total volume of the gases is 20L, what is the percent yield for this process?  EMBED Equation.3  8. Very hot zinc will react with steam to form zinc oxide and hydrogen. 5.4L of H2 was used to use up 20.0 g of zinc completely? What is the percent yield of this process?  EMBED Equation.3  WS E Molar Mass Worksheet KEY Name _________________ 2.35g of metal with a charge of +2 reacts with hydrochloric acid to produce 0.598 L of gas at STP. What metal do you have?  EMBED Equation.3  (NH4)3PO4 reacts with 0.0345 g of metal sulfate (M2(SO4)3) to produce 0.0399 g of (NH4)2SO4. Balance the equation. What is the molar mass of the metal? What is the metal? __M2(SO4)3 + 2(NH4)3PO4 ( 3(NH4)2SO4 + 2MPO4 0.0345g 0.0456g  EMBED Equation.3   EMBED Equation.3  3.45g of a metal hydroxide with charge + 1 reacts with excess Iron III Chloride to make 0.82g of Iron III hydroxide. What is the identity of the metal hydroxide?  EMBED Equation.3  30.2L of oxygen is produced at STP when 135.9 g of metal chlorate of charge +3 decomposes into oxygen and the metal chloride. What is the identity of the metal chlorate?  EMBED Equation.3  Mixed Stoichiometry Worksheet KEY 1. How many grams of water are formed when 12.5-g of hydrogen reacts with oxygen? 2H2+O2(2H2O12.5g?g EMBED Equation.3  2. How many liters of carbon dioxide are formed when 12.3-g of sodium carbonate reacts with 2.0-L of hydrogen chloride. The reaction is printed below: Na2CO3 + HCl ( NaCl + H2O + CO2 Na2CO3+2HCl(2NaCl+ H2O + CO212.3g2.0LL? EMBED Equation.3  3. How many grams of precipitate are formed when 24.3-g of zinc nitratre reacts with 20.5-g of sodium phosphate? 3Zn(NO3)2+2Na3PO4(Zn3(PO4)2+6NaNO324.3g20.5g?g (ppt) EMBED Equation.3  4. How many liters of oxygen are produced when 3.25-g of KClO3 decomposes into KCl and O2? 2KClO3(2KCl+3O23.25gL? EMBED Equation.3  5. When 2.25-g of sodium chloride reacts with excess silver nitrate, 3.45-g of precipitate is formed. What is the percent yield? NaCl+AgNO3(AgCl+NaNO32.25g3.45g EMBED Equation.3  6. 4.35-g of C5H12 reacts with 4.0-L of O2. a. How many liters of CO2 are formed? b. How much excess reactant remains? C5H12+8O2(5CO2+6H2O4.35g4.0LL? EMBED Equation.3  7. 3.0-g of zinc reacts with silver nitrate to form how many grams of zinc nitrate? Zn+2AgNO3(Zn(NO3)2+2Ag3.0g?grams? EMBED Equation.3  8. 8.2-mol of barium carbonate decomposes into how many moles of barium oxide. The other product is carbon dioxide. BaCO3(BaO+CO28.2mol?mol EMBED Equation.3  9. 4.5-g of sodium hydroxide reacts with 2.0-g of sulfuric acid (H2SO4). How many grams of water are formed? 2NaOH+H2SO4(2HOH+Na2SO44.5g2.0gG? EMBED Equation.3  10. 8.0-L of butane (C4H10) reacts with oxygen to make 50-g of carbon dioxide. What is the percent yield? 2C4H10+13O2(8CO2+10H2O8.0L50g EMBED Equation.3  11. 8.5-L of hydrogen reacts with 5.4-L of nitrogen to make a. how many liters of ammonia (NH3)? b. How many liters of excess reactant remains? 3H2+1N2(2NH38.5L5.4L?L EMBED Equation.3  12. ** 2.25-g of aluminum sulfate reacts with 3.25-g of sodium phosphate to make 1.0-g of precipitate. What is the percent yield? Al2(SO4)3+2Na3PO4(2AlPO4+3Na2SO42.25g3.25g1.0g This is both a limiting reactant problem and a percent yield problem  EMBED Equation.3  Chapter 10 Review EHS Chemistry 1. 23.5-g of KClO3 decomposes in the following way: KClO3 ( KCl + O2 How many grams of O2 was forms? (Make sure to balance the equation) 2. In the reaction: Na2CO3 + H3PO4 ( Na3PO4 + H2O + CO2 How many grams of Na2CO3 react with the H3PO4 to produce 100L of CO2 at STP? 3. Mercury (II) oxide decomposes to form liquid mercury and oxygen gas. If 5.4 g of mercury (II) oxide decomposes, how many grams of mercury is formed? (Hint: You must start with a correctly balanced chemical reaction) 4. 2.5-g of C4H10 reacts with 0.59-L of O2 at STP to form CO2 and H2O. a. Write the balanced equation. b. How many grams of H2O will be formed? c. How much excess reactant remains? 5. 2.30-g of Barium chloride reacts with 5.45-g of sodium carbonate in a double displacement reaction. How many grams of precipitate will form? (Hint: These are the calculations for the lab that you did). Make sure to use the table of solubilites to determine which substance is the solid precipitate. 6. 32.5-g of Hg(NO3)2 reacts with NH4Cl to make HgCl2 and NH4NO3. When the chemicals were mixed it was discovered that 20.0-g of HgCl2 was formed. What is the percent yield? 7. BONUS: 2.52x1025 atoms of sodium react with 325-L of phosphoric acid gas (H3PO4) at STP. 302.5-L of a gas is given off. What is the percent yield of the reaction? Chapter 10 Review KEY EHS Chemistry 1. 23.5-g of KClO3 decomposes in the following way: KClO3 ( KCl + O2 How many grams of O2 was forms? (Make sure to balance the equation) 2KClO3( 2KCl+3O223.5gG? EMBED Equation.3  2. In the reaction: Na2CO3 + H3PO4 ( Na3PO4 + H2O + CO2 How many grams of Na2CO3 react with the H3PO4 to produce 100L of CO2 at STP? 3Na2CO3+2H3PO4(2Na3PO4+3HOH+3CO2?g100L EMBED Equation.3  3. Mercury (II) oxide decomposes to form liquid mercury and oxygen gas. If 5.4 g of mercury (II) oxide decomposes, how many grams of mercury is formed? (Hint: You must start with a correctly balanced chemical reaction) 2HgO(2Hg+O25.4g?g EMBED Equation.3  4. 2.5-g of C4H10 reacts with 0.59-L of O2 at STP to form CO2 and H2O. a. Write the balanced equation. b. How many grams of H2O will be formed? c. How much excess reactant remains? 2C4H10+13O2(8CO2+10H2O2.5g0.59L?g EMBED Equation.3  5. 2.30-g of Barium chloride reacts with 5.45-g of sodium carbonate in a double displacement reaction. How many grams of precipitate will form? (Hint: These are the calculations for the lab that you did). Make sure to use the table of solubilites to determine which substance is the solid precipitate. BaCl2+Na2CO3(BaCO3+2NaCl2.30g5.45g?g:ppt EMBED Equation.3  6. 32.5-g of Hg(NO3)2 reacts with NH4Cl to make HgCl2 and NH4NO3. When the chemicals were mixed it was discovered that 20.0-g of HgCl2 was formed. What is the percent yield? Hg(NO3)2+2NH4Cl(HgCl2+2NH4NO332.5g20.0g EMBED Equation.3  7. BONUS: 2.52x1025 atoms of sodium react with 325-L of phosphoric acid gas (H3PO4) at STP. 302.5-L of a gas is given off. What is the percent yield of the reaction? 6Na+2H3PO4(2Na3PO4+3H22.52E25325L302.5L EMBED Equation.3  WS E Molar Mass Worksheet KEY Name _________________ (NH4)3PO4 reacts with 0.0345 g of metal sulfate (M2(SO4)3) to produce 0.0456 g of (NH4)2SO4. Balance the equation. What is the molar mass of the metal? What is the metal? __M2(SO4)3 + 2(NH4)3PO4 ( 3(NH4)2SO4 + 2MPO4 0.0345g 0.0456g  EMBED Equation.3   EMBED Equation.3  2.35g of metal with a charge of +2 reacts with hydrochloric acid to produce 0.598 L of gas at STP. What metal do you have?  EMBED Equation.3  3.45g of a metal hydroxide with charge + 1 reacts with excess Iron III Chloride to make 0.82g of Iron III hydroxide. What is the identity of the metal hydroxide?  EMBED Equation.3  30.2L of oxygen is produced at STP when 135.9 g of metal chlorate of charge +3 decomposes into oxygen and the metal chlorate. What is the identity of the metal chloride?  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2@BzHwP8`!@BzHwP8^ C2` gxڝ?oP{[&4$T- PNf<:v@@dR  &` @0XXX}NHҴKwν#`wB-TbN a UeEJ ѯl !$!5`Wfi颮G=- ;TrÍE|~} }*/[n;MgҶj ԉ\Pcjgnw5U%ئz~s}2{1Tf]%25aݗfvö]2# 6OV-epe3V97I6UW9sptb̆]]N>DGyQ0).p|T9> j 咺>,(&REb: n+KWU'SYܥW9YŰ/>aSU vG8Lxר8%o΀<裯>q?u34M78'̈ OL<8Z;h=<<zyxq`ⶥzxR3<y T[񤉋ǩِE?s>jtvDu߭HL[hGHC{CS7Ǐ C2` xVoT>գVV . 8(*B u/0 ǵؑvʤfAS@/7ަ{#*$:9;wιDZyp\lÕp0wsUuuK]1O0;'Q0Ĕ?مW=P`"{ 0M%cͰaTWȡQkpsGa0'n;$zk=kKA_!Lru"շ~{3ųC*5V}duB9ݶ%^7ϑ 0͵U0jU)V ux4{DVm^c ִiXX[y+ #\E2D*M˃$ћ_,JRBq4 |Q|+1nە{)J5珄Qw\Ҳ7S᧬6T"~iObjInfo]Equation Native V_979681454J|`F0˶pf0˶pfOle 4:4 CuSO 4 +Ba(NO 3 ) 2 !BaSO 4  (s) +Cu(NO 3 ) 2  (aq) 43.5g                             g?43.5gCuSO 4 1x1molCuSO 4 159.5gCuSO 4 x1molBaSO 4 1molCuSO 4 x233gBaSO 4 1molBaSO 4 =63.5gBaSO 4FMicrosoft EquationDNQE ECompObj_aRObjInfobEquation Native _1257847680eF0˶pf0˶pfquation.3 Ca+H 2 SO 4 CaSO 4 +H 2 13.5g                                ?L13.5gCa1x1molCa40gCax1molH 2 1molCax22.4LH 2 1molH 2 =7.6LH 2 FMicrosoft Equation 3.0 DS Equation Equation.39qgX( Zn+2HNO 3 !Zn(NO 3 ) Ole CompObjdffObjInfogEquation Native 2 +H 2 ?g                                       45.6L45.6LH 2 1x1molH 2 22.4LH 2 x1molZn1molH 2 x65gZn1molZn=132gZn FMicrosoft Equation 3.0 DS Equation Equation.39qžH, 2Cs+2H 2 O!2CsOH+H 2 14.5g           _1257847704rjF0˶pf0˶pfOle CompObjikfObjInfolEquation Native _979680601oF0˶pf0˶pfOle CompObjnpN                     ?molec14.5gCs1x1molCs133gCsx1molH 2 2molCsx6.02x10 23 molecH 2 1molH 2 =3.28x10 22 molecH 2FMicrosoft EquationDNQE Equation.3! 2Ag+Cl 2 2AgCl84gAgCl1x1molAgCl143.5gAgClx2molAg2molAgClx10ObjInfoqEquation Native =_1257927740tF0˶pf0˶pfOle 8gAg1molAg=63.2gAg FMicrosoft Equation 3.0 DS Equation Equation.39q43/ 7.5LH 2 1x1molH 2 22.4LH 2 x1moCompObjsufObjInfovEquation Native O_979704416yF0˶pf0˶pf     !"%()*+,-./256789<?@ABCFIJKLORSTUVWX[^_`abcdefghijklmnopqtwxyz{|}~lZn1molH 2 x65gZn1molZn=21.8gZnFMicrosoft EquationDNQE Equation.3R 5.6gFeOle CompObjxzNObjInfo{Equation Native n1x1molFe56gFex3molCl 2 2molFex6.02x10 23 molecCl 2 1molCl 2 =9.03x10 22 molecCl 2FMicrosoft EquationDNQE Equation.3_979704745w~F0˶pf0˶pfOle  CompObj}NObjInfoz 2.1x10 24 molecO 2 1x1molO 2 6.02x10 23 molecO 2 x4molNH 3 7molO 2 x17gNH 3 1molNH 3 =33.9gNH 3Equation Native _979705022F0˶pf0˶pfOle CompObjNFMicrosoft EquationDNQE Equation.3y 250gC 5 H 12 1x1molC 5 H 12 72gC 5 H 12 x5molCO 2 1molCObjInfoEquation Native _1226294306F0˶pf0˶pfOle # 5 H 12 x22.4LCO 2 1molCO 2 =389LCO 2 FMicrosoft Equation 3.0 DS Equation Equation.39qaH6t 5.5LNCompObj$fObjInfo&Equation Native '._979705425^"F0˶pf0˶pf 2 O 3 1x1molN 2 O 3 22.4LN 2 O 3 x3molO 2 2molN 2 O 3 x6.02x10 23 molecO 2 1molO 2 =2.2x10 23 moleculesO 2Ole 0CompObj1NObjInfo3Equation Native 4^FMicrosoft EquationDNQE Equation.3B 2.53gAgNO 3 1x1molAgNO 3 170gAgNO 3 x1molAgCl1molAgNO 3 x143.5gAgCl1molAgCl=2.14gAgClFMicrosoft EquationDNQE Equation.3? 50.6LCH 4 1x1molCH 4 2_979705594F0˶pf0˶pfOle :CompObj;NObjInfo=Equation Native >[_979705757F0˶pf0˶pfOle DCompObjEN2.4LCH 4 x1molCO 2 1molCH 4 x44gCO 2 1molCO 2 =99.4gCO 2FMicrosoft EquationDNQE Equation.3ObjInfoGEquation Native H3_979705920F0˶pf0˶pfOle M 45.5gCaO1x1molCaO56gCaOx1molCO 2 1molCaOx22.4LCO 2 1molCO 2 =18.2LCO 2FMicrosoft EquationDNQE Equation.3CompObjNNObjInfoPEquation Native Q_1041763432F0˶pf0˶pf 3.25gCu(NO 3 ) 2 1x1molCu(NO 3 ) 2 187.5gCu(NO 3 ) 2 x1molCu(OH) 2 1molCu(NO 3 ) 2 x97.5gCu(OH) 2 1molCu(OH) 2 =1.69gCu(OH) 2FMicrosoft Equation 3.0DNQE Equation.3 2Fe+3Cl 2 2FeCl 3 114g   292.7g      ?g114gFOle YCompObjZRObjInfo\Equation Native ] e1x1molFe56gFex2molFeCl 3 2molFex162.5gFeCl 3 1molFeCl 3 =331gFeCl 3 292.7gCl 2 1x1molCl 2 71gCl 2 x2molFeCl 3 3molCl 2 x162.5gFeCl 3 1molFeCl 3 =447gFeCl 3 Fe is the LR because it yielded the smallest answer114gFe1x1molFe56gFex3molCl 2 2molFex71gCl 2 1molCl 2 =217gCl 2 used up292.7-217g=75.9gCl 2 leftFMicrosoft Equation 3.0DNQE Equation.3 2CH 3 OH+3O 2 2CO 2 +4H      5-" !#&$%'(),*+.1/0234uv6789:;<=>?@ABCDEFGHIJKLMNOPQRSTUVWXYZ[\]^_`abcdefghijklmnopqrstwxyz{|~}z_UbV.;{qԥ(ӮI16m(i|a6m02;)iy$jq!6#sL2)i3=M~>J1ZsVZZiAx&!d,qǮi ј՛0|[ewDk֨_¶i'̔T;v+~)<|3;Q6y4ղ*JC摿$ *Yxd!yFS&Oks(c5m5"4m.悹YCqWBrN(UCVjZEcd4q2׎̩^e>ϸ8w5 Bլyh )4撧+r*G`nxpݠKgCxz&>HQ%0.O<)OʓH}KpE5X'O8AbȔ'52G!cSzdl1' !ҍOd1S<'!f>Ski/ uFq2eyI 2lZ'bX\ Dd l~|h  s *A? 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N 2 H 4 +2H 2 O 2 N 2 +4H 2 O25g           66g        g?                      25gN 2 H 4 1x1molN 2 H 4 32gN 2 H 4 x1molN 2 1molN 2 H 4 x28gN 2 1molN 2 =22gN 2 66gH 2 O 2 1x1molH 2 O 2 34gH 2 O 2 x1molN 2 2molH 2 O 2 x28gN 2 1molN 2 =27gN 2 N 2 H 4  is the LR because it yielded the smallest answer25gN 2 H 4 1x1molN 2 H 4 32gN 2 H 4 x2molH 2 O 2 1molN 2 H 4 x34gH 2 O 2 1molH 2 O 2 =53gH 2 O 2 66g-53g=13gH 2 O 2 leftoverFMicrosoft Equation 3.0DNQE Equation.3 6Li+Al CompObjRObjInfoEquation Native +_1041749905F0˶pf0˶pf2 (SO 4 ) 3 3Li 2 SO 4 +2Al22.5g         33.5             g?                      22.5gLi1x1molLi7gx3molLi 2 SO 4 6molLix110gLi 2 SO 4 1molLi 2 SO 4 =177gLi 2 SO 4 33.5gAl 2 (SO 4 ) 3 1x1molAl 2 (SO 4 ) 3 342gAl 2 (SO 4 ) 3 x3molLi 2 SO 4 1molAl 2 (SO 4 ) 3 x110gLi 2 SO 4 1molLi 2 SO 4 =32gLi 2 SO 4 Al 2 (SO 4 ) 3  is the LR since it yields the smaller value33.5gAl 2 (SO 4 ) 3 1x1molAl 2 (SO 4 ) 3 342gAl 2 (SO 4 ) 3 x6molLi1molAl 2 (SO 4 ) 3 x7gLi1molLi=4.1gLi22g-4.1g=18gLiLeftoverFMicrosoft Equation 3.0DNQE Equation.3Ole CompObjRObjInfoEquation Native  SO 2 +H 2 OH 2 SO 3 33.6g  55.3g     g?                      33.6gSO 2 1x1molSO 2 64gSO 2 x1molH 2 SO 3 1molSO 2 x82gH 2 SO 3 1molH 2 SO 3 =43gH 2 SO 3 55.3gH 2 O1x1molH 2 O18gH 2 Ox1molH 2 SO 3 1molH 2 Ox82gH 2 SO 3 1molH 2 SO 3 =252gH 2 SO 3 SO 2  is the LR since it yields the smaller value33.6gSO 2 1x1molSO 2 64gSO 2 x1molH 2 O1molSO 2 x18gH 2 O1molH 2 O=9.5gH 2 O55.3g-9.5g=45.8gH 2 OLeftover_1041763970F0˶pf0˶pfOle CompObjRObjInfoFMicrosoft Equation 3.0DNQE Equation.3 2KI+Pb(NO 3 ) 2 PbI 2 +2KNO 3 77g       32g              g?      Equation Native _1003557485F0˶pf0˶pfOle CompObjR                77gKI1x1molKI166gKIx1molPbI 2 2molKIx461gPbI 2 1molPbI 2 =107gPbI 2 32gPb(NO 3 ) 2 1x1molPb(NO 3 ) 2 331gPb(NO 3 ) 2 x1molPbI 2 1molPb(NO 3 ) 2 x461gPbI 2 1molPbI 2 =45gPbI 2 Pb(NO 3 ) 2  is the LR since it yields the smaller value32gPb(NO 3 ) 2 1x1molPb(NO 3 ) 2 331gPb(NO 3 ) 2 x2molKI1molPb(NO 3 ) 2 x166gKI1molKI=32gKI77g-32g=45gKILeftoverFMicrosoft EquationDNQE Equation.3ObjInfoEquation Native >_979850155F0˶pf0˶pfOle      "#$%&'*-./256789:;<=>ADEFGHIJKLORSTUVWXYZ[\_bcdefghijklmnoruvwxyz{~" 4NH 3 +7O 2 6H 2 O+4NO 2 22L      19L                       L?      I got 19L of air by mulitplying 95L of air by 20%                22LNH 3 1x4LNO 2 4LNH 3 =22LNO 2 19LO 2 1x4LNO 2 7LO 2 =11LNO 2 O 2  is the LR since it yields the smaller value19LO 2 1x4LNH 3 7LO 2 =11LNH 3 22L-11L=11LNH 3 LeftoverFMicrosoft EquationDNQE Equation.3 15.5gNH 4 Cl1x1molNH 4CompObjNObjInfoEquation Native _979850415F0˶pf0˶pf Cl53.5gNH 4 Clx1molAgCl1molNH 4 Clx143.5gAgCl1molAgCl=41.57gAgCl%=35.5g41.57gx100=85.3%FMicrosoft EquationDNQE Equation.3Ole CompObjNObjInfo Equation Native ! 32.5gKClO 3 1x1molKClO 3 122.5gKClO 3 x2molKCl2molKClO 3 x74.5gKCl1molKCl==19.7gKCl%=15.2g19.7gx100=76.9%ѷoһQ$QN8~|\5WzV\& SԔx))8O#btj4%UxLnk+򛼢j3cig8 >v1Oȟ˹嬔)zVk_+/ 4_߯Z4Uu)*0=lMXm|S* N7w@SE\WS\-OO/|=XE>?C޹7C_M] nT FG^wi?$TCнO=;ptUEedk$]*|]Jv{ApAhkH(uA (0]Pd܏e :B]Xhp/2Wz0Ca07 XbPPeP e\La+χi,EE @,U$xQ:SRD ,WT8?,WZ <dC8%:7yHª/+-*+ҟp56q)K= pH ݂kЈ0H[1KNLe(C x4W_p96}~sIc53>QP~P@h#cEݦ"*|m{m$AQʒN1NuaInx{*xA6'aF078]> abMl.k'P Vu͟* *~ u[4B4FQ[燤w޼=b-[6|#+ e'6٩M"5D&7j^E^-r?1mbcޮ=c=ߛX +/2Ųc#%#69ԀV&@{2>kN*(x3=McB4r՛#WMf67q>&5}"svH}7W[exfcCSmQm0rDvJX[;\>zry'ᑃtX_tfnPMϻZ )B4~^ďjx"함xh-ƕ:,҃63 8#Q&#YUXG;u3 |zEl( ntS҉tMkdW]쬎)֘<كoffM]nH߀eⴜDXqFJ3\*/t]q:rI9h=N#Z2"v8# ZOp-Du:6|){Hk $(;־JԨXsypӱsm^ޱ 9'wݹ^&??95a~{ ^ˊ5uYRje}\-buϊX]fq3e+YhɟI"7kuQ.!i.5}BVS k5586JIi/1 P))\d'JiɯJI/ssi 7 K Jп+hG |8s#qxw\ÚW:cPnE+V>Wyg3u4+'jԙQ'xg?W+rɍsGEXYl5uS0saCx &g"ܼT40!UxXo$Gn;gPig{jJ8AHxg=xcM0A31ڬ'"qZH'n$.\W]7F6i>OA>V?,C&C~+ ']YIzm )418L(.:wtx9'q,. 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