аЯрЁБс;ўџ ўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџ§џџџ ўџџџ ўџџџўџџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџRџџџџџџџџ РFEѕаМО@CompObjџџџџџџџџџџџџ\WordDocumentџџџџџџџџ rObjectPoolџџџџ€Ў\аМО€Ў\аМОўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџ>?@ABCDўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџўџџџџџ РFMicrosoft Word 6.0 DocumentўџџџNB6WWord.Document.6;џў џџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџмџџџнџџџоџџџпџџџрџџџсџџџтџџџуџџџфџџџхџџџцџџџчџџџшџџџщџџџъџџџык зм0€зм№зЉ€Ћ€ ’”   џ>89џP 7џX 79џџзм€[`Ц ˆзкРрзЉ€EdFAABАЪ зкРзмаРзь№ЫœЫ Ы|зкРЫXЪŸаЪŸ@ЪžАЪž ЪаЪ@ЪœАЪœ Ъ›Ъ›@ЪšАЪš Ъ™Ы|зLab: The Sulfur Clock Reaction  Introduction If you examine the different chemical reactions you have done in the lab this year, you will notice that they have taken different amounts of time to occur. In this lab, we will examine the rates (kinetics) of chemical reactions. We will look at the relationship of time and speed of a reaction and finally, we will examine the effect of changing concentrations on the time it takes for a chemical reaction to occur. MATERIALS: 1 well plate distilled water 0.15 M sodium thiosulfate (Na2S2O3) solution 1 micropipet 1 M hydrochloric acid (HCl) 1 small glass rod Procedure 1. Prepare the well plate with water and thiosulfate as shown in the data table. 2. On a piece of paper, use a pencil to make 8 small вxеsг that can be placed underneath each of the 8 wells. 3. Now place 2 drops of HCl solution in well 1 and stir once with the small glass rod. Begin timing the reaction from the moment you add the acid. Finish timing when the reaction causes the вxг to be obscured. 4. Now place 2 drops of HCl, stir and time. Continue this procedure until all 8 wells have been reacted with 2 drops of HCl and timed. 5. Clean the well plate and wash your lab bench. Data DROPS OF 0.15 M NA2S2O3DROPS OF WATERTIME (seconds)SPEED (1/t)WELL 1100WELL 291WELL 382WELL 473WELL 564WELL 655WELL 746WELL 837 Calculations 1. Calculate the speed of each reaction and record it in the data table. Analysis 1. Prepare a graph by plotting time on the y-axis and the number of drops of thiosulfate on the x-axis. 2. What is the relationship between the concentration of thiosulfate and the time it takes for a reaction to occur? 3. What is the difference between time and speed or rate? 4. Prepare a second graph of speed on the y-axis and the number of drops of thiosulfate on the x-axis. 5. What is the relationship between the concentration of thiosulfate and the speed of the reaction? KINETICS Name: _______________________ Partner #1: _______________________ Partner #2: _______________________ Acton-Boxborough Regional High School Due Date: ______________________ Acton-Boxborough Regional High School Ž™?І Ї ЈаЉа|HHк(џсџсљEG(ќHHк(d'`ŽžІ Ї ЈаЉа|HHк(џсџсљEG(ќHHк(d'`Ž™ І Ї ЈаЉа|HHк(џсџсљEG(ќHHк(d'`00&tњa0`0(00&ќљйи00&ќљЁйи00&ќљйи00&ќљŒйи00&ќљŽйиаЯрЁБсўџ ђŸ…рOљhЋ‘+'Гй0Ѓ˜ь& , 8 DPX `l‰ ‘›SummaryInformation(џџџџџџџџџџџџ=гџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџўџџџLScience F:Applications:Microsoft Office:Microsoft Word 6:Templates:chem labLAB: TITLE OF LABsciencescience'@”Щ?цЛО@PjЅчЛО@,cЎМО@Microsoft Word 6.0.15;џў џџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџмЅhOР eр rђэооооооо4VVVVV(~ ˆVFVЄЄЄЄЄффф      &œXє~Fоф Є@фффFфооЄЄффффоЄоЄ 6оооофф:фLab: The Sulfur Clock Reaction  Introduction If you examine the different chemical reactions you have done in the lab this year, you will notice that they have taken different amounts of time to occur. In this lab, we will examine the rates (kinetics) of chemical reactions. We will look at the relationship of time and speed of a reaction and finally, we will examine the effect of changing concentrations on the time it takes for a chemical reaction to occur. MATERIALS: 1 well plate distilled water 0.15 M sodium thiosulfate (Na2S2O3) solution 1 micropipet 1 M hydrochloric acid (HCl) 1 small glass rod Procedure 1. Prepare the well plate with water and thiosulfate as shown in the data table. 2. On a piece of paper, use a pencil to make 8 small вxеsг that can be placed underneath each of the 8 wells. 3. Now place 2 drops of HCl solution in well 1 and stir once with the small glass rod. Begin timing the reaction from the moment you add the acid. Finish timing when the reaction causes the вxг to be obscured. 4. Now place 2 drops of HCl, stir and time. Continue this procedure until all 8 wells have been reacted with 2 drops of HCl and timed. 5. Clean the well plate and wash your lab bench. Data DROPS OF 0.15 M NA2S2O3DROPS OF WATERTIME (seconds)SPEED (1/t)WELL 1100WELL 291WELL 382WELL 473WELL 564WELL 655WELL 746WELL 837 Calculations 1. Calculate the speed of each reaction and record it in the data table. Analysis 1. Prepare a graph by plotting time on the y-axis and the number of drops of thiosulfate on the x-axis. 2. What is the relationship between the concentration of thiosulfate and the time it takes for a reaction to occur? 3. What is the difference between time and speed or rate? 4. Prepare a second graph of speed on the y-axis and the number of drops of thiosulfate on the x-axis. 5. What is the relationship between the concentration of thiosulfate and the speed of the reaction? 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