Largest Source Of Error In Calorimetry Experiment
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How To Improve Calorimeter Experiment
Businesses News & Events Pets Politics & Government Pregnancy & Parenting Science & Mathematics Social Science systematic error calorimetry Society & Culture Sports Travel Yahoo Products International Argentina Australia Brazil Canada France Germany India Indonesia Italy Malaysia Mexico New Zealand Philippines Quebec Singapore Taiwan Hong likely errors in colorimetry Kong Spain Thailand UK & Ireland Vietnam Espanol About About Answers Community Guidelines Leaderboard Knowledge Partners Points & Levels Blog Safety Tips Science & Mathematics Physics Next What are the Errors in a calorimeter lab? We did a lab proving the conservation of thermal energy using a calorimeter. Our objective was that
Calorimeter Lab Report
the heat lost by hot water was the heat gained by the cold water. My group got 20% error!! What are the possible sources of it? 2 following 4 answers 4 Report Abuse Are you sure you want to delete this answer? Yes No Sorry, something has gone wrong. Trending Now Marla Maples Harry Shearer Emirates airlines Great Barrier Reef 2016 Crossovers Cable TV Annette Bening Ellen DeGeneres Subaru Forester Malik Obama Answers Relevance Rating Newest Oldest Best Answer: The easiest error reason is that the calorimeter wasn't a perfect insulator. This is because you must have opened the calorimeter when you added the cold water. Thus, heat was lost not only to the cold water but to the surrounding environment. Also, you might not have waited long enough for the thermometer to read, so the temperature of the hot water was lower than it really was, or the temperature of the cold water
Education Science Chemistry main sources of error in calorimetry Results 1 to 7 of 7 Thread: main sources of error in calorimetry LinkBack LinkBack URL About LinkBacks Bookmark & Share Digg this Thread!Add calorimetry lab conclusion Thread to del.icio.usTweet this threadShare on FacebookReddit! Thread Tools Show Printable Version Email calorimetry physics this Page… Subscribe to this Thread… Rate This Thread Current Rating Excellent Good Average Bad Terrible 17 Sep 2003,6:48 PM #1
What Is Calorimetry
ignition Guest main sources of error in calorimetry Can someone please tell me what the main significant sources of error that would come from in a calorimetry experiment? Reply With Quote 17 Sep https://answers.yahoo.com/question/?qid=20070601100622AA6Z8ot 2003,6:58 PM #2 jm1234567890 Rambling Spirit Join Date Aug 2002 HSC 2003 Gender Male Location Stanford, CA Posts 6,524 Rep Power 15 heat loss to environment Share Share this post on Digg Del.icio.us Twitter Facebook Reddit! Telecommunications Engineering/Maths @ University of Wollongong [University Medal] MSc/PhD Electrical Engineering [Computational Biology] @ Stanford University Check out SpliceMap! Reply With Quote 17 Sep 2003,7:03 PM #3 hipsta_jess Up the mighty http://community.boredofstudies.org/17/chemistry/12133/main-sources-error-calorimetry.html red V Join Date May 2003 HSC N/A Gender Female Posts 5,991 Rep Power 13 Originally posted by jm1234567890 heat loss to environment yep, from around the bunsen and above the holding container thing. Share Share this post on Digg Del.icio.us Twitter Facebook Reddit! Reply With Quote 17 Sep 2003,7:14 PM #4 jm1234567890 Rambling Spirit Join Date Aug 2002 HSC 2003 Gender Male Location Stanford, CA Posts 6,524 Rep Power 15 also lack of stiring Share Share this post on Digg Del.icio.us Twitter Facebook Reddit! Telecommunications Engineering/Maths @ University of Wollongong [University Medal] MSc/PhD Electrical Engineering [Computational Biology] @ Stanford University Check out SpliceMap! Reply With Quote 17 Sep 2003,7:29 PM #5 jayz walking Join Date Jun 2003 Location inner west Posts 473 Rep Power 10 Originally posted by jm1234567890 also lack of stiring do u mean-lack of even heating? Share Share this post on Digg Del.icio.us Twitter Facebook Reddit! risk hunting Reply With Quote 20 Sep 2003,3:45 PM #6 CHUDYMASTER Master of Chudy 'n' Curry Join Date Oct 2002 HSC 2001 Gender Undisclosed Posts 568 Rep Power 11 The obvious one is heat losses to the air and to the beaker (essentially one point), but the one people te
thermometer, 400-mL beaker, 250-mL beaker, 50-mL graduated cylinder You need these materials: 1 M HCl, 1 M HC2H3O2 (acetic acid), 1 M NaOH Every chemical change is accompanied by a change in energy, usually in the form of heat. The energy change of a http://www.yaksic.com/hn26.html reaction that occurs at constant pressure is termed the heat of reaction or the enthalpy https://www.coursehero.com/file/10632775/Heat-of-Naturalization-Lab/ change. If heat is evolved, the reaction is exothermic. If heat is absorbed, the reaction is endothermic. So let's do an experiment together! We will observe two exothermic reactions, and find the heat of reaction for each. The reaction studied will be the heat of neutralization, which is the enthalpy change produced when an acid and a base react to of error form water. In order to measure the amount of heat produced by a reaction, an instrument called a calorimeter must be used. The calorimeter used in this experiment will be somewhat rudimentary. It will be constructed as shown in the following picture: (view | download) This calorimeter consists of two polystyrene cups nested together, which are then placed in a 400-mL beaker. A cardboard square is added on top to keep heat inside the calorimeter and largest source of to stabilize the thermometer which juts out of the cardboard into the solution below. The heat liberated in the neutralization reaction occurring within the calorimeter will cause an increase in the temperature of the solution and of the calorimeter. If the calorimeter were perfect, no heat would be radiated to the laboratory. Two forms of enthalpy must be measured in this experiment: the heat that causes a temperature increase in the solution and the heat that causes a temperature increase in the calorimeter. In order to determine the amount of heat absorbed by the calorimeter, we must first determine the heat capacity of the calorimeter. The heat capacity is the amount of heat required to raise its temperature by 1 Kelvin, or 1 degree Celsius, which are equivalent increments. However, the heat capacity must be found using standard solutions. In this case, tap water will be used to find the heat capacity of the calorimeter as outlined in the Procedure. In order to interpret the data obtained, two final steps must be taken. All of the temperatures observed by the thermometer must be adjusted according to the calibration curve. But if you don't know how to make your own calibration curve, you're shit out of luck! I can't tell you anything about it. Also, we must find the change in temperature of a solution to d
Upload Documents Write Course Advice Refer your Friends Earn Money Upload Documents Apply for Scholarship Create Q&A pairs Become a Tutor Find Study Resources by School by Literature Guides by Subject Get Instant Tutoring Help Ask a Tutor a Question Use Flashcards View Flashcards Create Flashcards Earn by Contributing Earn Free AccessLearn More > Upload Documents Write Course Advice Refer your Friends Earn MoneyLearn More > Upload Documents Apply for Scholarship Create Q&A pairs Become a Tutor Are you an educator? Log in Sign up Home Albany State University CHM CHM 113 Heat of Naturalization Lab Heat of Naturalization Lab - Andrew Rosen Mrs. Davidson... SCHOOL Albany State University COURSE TITLE CHM 113 TYPE Lab Report UPLOADED BY dsadsa231 PAGES 4 Click to edit the document details This preview shows pages 1–2. Sign up to view the full content. View Full Document Andrew Rosen Mrs. Davidson Period 6/7 December 14 th , 2009 Heat of Neutralization Lab Questions: 1) What is the largest source of error in the experiment? The largest source of error in this experiment was probably the amount of solution added to the calorimeter. At times, human error made it so the amount was not exactly 50.0mL like the lab dictates. Also, during this lab, the solution was not mixed frequently and this could have caused inaccurate temperature readings and thus make the results askew. 2) How should the two heats of reaction for the neutralization of NaOH and the two acids compare? Why? The two heats of reaction for the neutralization of NaOH and the two acids should be rather similar because the same amounts of moles of NaOH are added to both acids. This should naturally cause the temperature difference () to be equal. The individual initial and final temperatures, however, can be different. The moles of products are all equal as well. This also should hold true since both HCl and HC 2 H 3 O 2 are strong acids/electrolytes. 3) The experimental procedure has you wash your thermometer and dry it after you measure the temperature of NaOH solution and before you measure the temperature of the HCl This preview has intentionally blurred sections. Sign up to view the full version. View Full Document This is the end of the preview. Sign up to access the rest of the document. TERM Winter '13 PROFESSOR Briggs TAGS Chemistry, Neutralization Click to edit the document detai