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Human Activity and Climate Change
In 3-4 pages, using APA-style formatting, discuss and give your position on the following statement: “Human activity, especially the burning of fossil fuels, is a major contributor to climate change”. Do you agree or disagree? Support your views with credible data. This is an area where junk science abounds. Be prepared to give and defend your sources as scientifically trustworthy.
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Riverside City College Chemistry Writing and Balancing Chemical Equations Exercises
writing ionic equations :1.Classify each of the compounds as a molecule or a salt.Molecule SaltAnswer bank :CaS, NO2, C2H5 ...
Riverside City College Chemistry Writing and Balancing Chemical Equations Exercises
writing ionic equations :1.Classify each of the compounds as a molecule or a salt.Molecule SaltAnswer bank :CaS, NO2, C2H5OH,KI,C6H6,CaSO42.Classify each of the ions as a cation or an anion.Cations AnionsAnswer bank : NO-/2, K+, Co3+,NH+4, Br-, OH-,SA2+,CO-/3, Ca2+, O2-3.Classify each of the ions as monoatomic or polyatomic.Monoatomic ions Polyatomic ionsAnswer bank : NO-2, OH-,Cu+, Be2+,S2-, H3O+, Sn2+, Na+,F-,O2/2-, CIO-/34.Balance the equations by inserting coefficients as needed.equation 1:PCl3+Cl2⟶PCl5equation 2:Mg3N2+HCl⟶MgCl2+NH35.Balance each equation by inserting coefficients as needed.equation 1:KHF2⟶KF+H2+F2equation 2:P4O10+H2O⟶H3PO46.Balance the chemical equation by adding coefficients as needed.equation: NaOH(aq)+NaNO2(aq)+Al(s)+H2O(l)⟶NH3(aq)+NaAlO2(aq)7.Write the formula for an ionic compound formed from the K+ ion and each additional ion.K+ and Cl− :K+ and N3− :K+ and S2− :8.Write the formula for an ionic compound formed from O2− with each of the ions.magnesium ion:sodium ion:aluminum ion:9.Predict the formula for a compound made from X2+ and Y2−.Insert subscripts as needed.formula: XY10.Give the formula for an ionic compound formed from each pair of ions.Na+ and O2−Al3+ and F−Mg2+ and S2−Ca2+ and P3−11.Determine the formula unit for the compound formed when each pairs of ions interact. Li+ and O2−:Mg2+ and S2−:Al3+ and Cl−:Na+ and N3−:12.Write the chemical formula for the compound formed by each pair of positive and negative ions.Ba2+ and NO3−:Al3+ and CO32−:K+ and PO43−: 13.Write the net ionic equation, including phases, that corresponds to the reactionZn(NO3)2(aq)+Na2S(aq)⟶ZnS(s)+2NaNO3(aq)net ionic equation:14.Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) and KCl(aq). Refer to the solubility rules as needed.net ionic equation:15.Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states.A. copper(II) sulfate, CuSO4, and potassium hydroxide, KOHnet ionic equation:B. lithium carbonate, Li2CO3, and aluminum nitrate, Al(NO3)3net ionic equation:C. sodium phosphate, Na3PO4, and barium chloride, BaCl2net ionic equation:17.Complete and balance the molecular equation for the reaction of aqueous iron(III) nitrate, Fe(NO3)3, and aqueous lithium hydroxide, LiOH. Include physical states.molecular equation:Fe(NO3)3(aq)+LiOH(aq)⟶Enter the balanced net ionic equation for the reaction. Include physical states.net ionic equation:18.Complete and balance the molecular equation for the reaction of aqueous sodium sulfate, Na2SO4, and aqueous barium nitrate, Ba(NO3)2. Include physical states.molecular equation:Na2SO4(aq)+Ba(NO3)2(aq)⟶Enter the balanced net ionic equation for this reaction. Include physical states.net ionic equation:19.Complete and balance the molecular equation for the reaction of aqueous sodium carbonate, Na2CO3, and aqueous nickel(II) chloride, NiCl2. Include physical states.molecular equation:Na2CO3(aq)+NiCl2(aq)⟶Enter the balanced net ionic equation for this reaction. Include physical states. net ionic equation:20.At temperatures above roughly 800 °C, calcium carbonate decomposes. Write and balance the equation for this reaction. Phase symbols are optional.21. For the chemical reaction2HBr(aq)+Ba(OH)2(aq)⟶2H2O(l)+BaBr2(aq)write the net ionic equation, including the phases.net ionic equation:22.Write the net ionic equation for the chemical reaction shown. Include physical states.HClO2(aq)+NaOH(aq)⟶H2O(l)+NaClO2(aq)net ionic equation:23.For the chemical reactionHClO4(aq)+NaOH(aq)⟶H2O(l)+NaClO4(aq)write the net ionic equation, including the phases.net ionic equation:Which ions are considered spectator ions for this reaction? H+ClO−4Na+OH−24.Complete and balance the equation for this single-displacement reaction. Phases are optional.equation:AgNO3+Al⟶25.Complete and balance the equation for the single-displacement reaction. Phases are optional.equation:Li+NaOH⟶26.Consider the decomposition reaction ? ⟶CaO(s)+CO2(g)
4 pages
20200927140105lab 7 Groundwater Worksheet
Save this document to your computer, fill in the information, and submit it via Canvas. Note that the worksheet will not b ...
20200927140105lab 7 Groundwater Worksheet
Save this document to your computer, fill in the information, and submit it via Canvas. Note that the worksheet will not be accepted for credit if the ...
University of Florida Drug Controlled Substance Hypothesis Statistical Lab Report
1. Write a Quality Assurance guide for the analysis of one of the following samples; both samples are suspected of having ...
University of Florida Drug Controlled Substance Hypothesis Statistical Lab Report
1. Write a Quality Assurance guide for the analysis of one of the following samples; both samples are suspected of having a drug, but have not undergone any testing as of yet:• A bag containing 100 grams of white powder suspected to contain a controlled substance (drug)OR100ml of human urine suspected to contain a controlled substance (drug)Please remember to address the following topics: scope, Terminology, Testing Facility, Personnel, QA Manual Documentation, Evidence Control, Chemical Reagents, Presumptive testing and confirmatory analytical Procedures, Validation, Equipment Maintenance and Calibration, Proficiency Testing, Audits, Deficiency of Analysis/Corrective Actions, and Health and Safety.Depending upon the analysis being performed, some items may not be applicable whereas other components may need to be added. Also, remember that you can reference a number of standard procedures (SOPs) by referring to established SOPs – you do not need to provide the specifics of the analysis but rather just an overview of the best practice to analyze the sample – which includes optimization of available resources such as analytical instruments and personnel. (20 points)The following FBI quality assurance guidelines summarize the essential goals and are helpful as a reference for this module as well as for the assignment:http://www.fbi.gov/about-us/lab/forensic-science-communications/fsc/jan2005/standards/2005standards15.htm (Links to an external site.)2. This following project involves the testing and comparison of quantitative results produced by two labs using two different analytical methods. A final report will need to be created following the completion of this project. Project Scenario: Two individual laboratories (Lab A and Lab B) were contracted to analyze 25 blood samples to determine the concentration of cocaine (and/or any metabolites) in each sample. Both labs used instrumentation that provided quantitative results, but each lab used a different method. Lab A utilized liquid chromatography- mass spectrometry (LCMS) and Lab B utilized gas chromatography-mass spectrometry (GCMS). For this project, each laboratory was tasked with analyzing the blood samples of 25 known cocaine users. As this project involved the comparison of Lab A with Lab B’s final results, each lab needed to analyze the same 25 samples. As these labs were located in different cities, two tubes of blood were drawn from each of the 25 subjects. One blood tube was sent to Lab A and the second was sent to Lab B so that each lab would have the same 25 samples to compare. Now that the testing has been completed, a final report needs to be created to address whether or not the results from the two laboratories are equivalent.For this assignment, you will need to write a brief outline for this project’s final report. This report should follow a clear structure and include all of the required components as described in the module’s reading. Be sure that the report you submit includes information on the two labs, the two different methods used, and 25 fictitious concentration results per lab. Additionally, be certain to include and explain all of the components that would be required for this final report as discussed in the reading. The concentration data must be included and a statistical analysis of that data must be included as a part of this report. Please consider the following when completing this assignment:* What does your fictional cocaine concentration data look like? You need to come up with your own fictional data for this assignment (the values for the concentrations should be in units of ng/mL). You must include the 25 concentration results for each lab as a part of the data as well as the results of the calculated statistics. You can simply present this concentration data in an Excel table or chart format* The statistical comparison needs to be calculated using either a student t-test or Wilcoxon. You must perform the statistical analysis on your fictional data and compare Lab A to Lab B. You must also provide a conclusion as to whether or not the two methods were comparable.Useful links:Cocaine analysis in various body fluids: https://www.researchgate.net/publication/14750172_Cocaine_and_benzoylecgonine_in_saliva_serum_and_urine (Links to an external site.)Research report guidelines: http://www.nlm.nih.gov/services/research_report_guide.html (Links to an external site.) You may also have to refresh some knowledge of statistical testing since you will be comparing two groups. Here is some reading material:“An Introduction to Statistics”, Driscoll P, Lecky F, Crosby M, J Accid Emerg Med, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725369/ (Links to an external site.)“An Introduction to hypothesis testing. Parametric comparison of two groups-1”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725552/ (Links to an external site.)“An Introduction to hypothesis testing. Parametric comparison of two groups-2”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725593/ (Links to an external site.) “An Introduction to hypothesis testing. Non-Parametric comparison of two groups-1”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725625/
4 pages
Bio Part 3
Directions for the students: There are 4 essay questions. Please be sure to complete all of them with thorough substantive ...
Bio Part 3
Directions for the students: There are 4 essay questions. Please be sure to complete all of them with thorough substantive responses. Citations are ...
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Lab Worksheet Module08
Use the Wave on a String Simulation for this lab. For this first simulation, click Pulse on the top left, and the rulers a ...
Lab Worksheet Module08
Use the Wave on a String Simulation for this lab. For this first simulation, click Pulse on the top left, and the rulers and timer on the bottom ...
Moraine Valley Community College Length Temperature and Mass Lab Report
Complete lab and fill out document attched with it.1Aluminum pie pan1Bottle of distilled water1Box of matches or lighter1D ...
Moraine Valley Community College Length Temperature and Mass Lab Report
Complete lab and fill out document attched with it.1Aluminum pie pan1Bottle of distilled water1Box of matches or lighter1DVD or CD4Dime1Fork1Isopropyl (rubbing) alcohol (C3H8O), 91%1Key1Pair of scissors1Pen or pencil5Penny1Plastic cup3Quarter1Sheet of white paper1Source of ice cubes1Source of tap water1Spoon1White granulated sugar (C12H22O11)HOL Supplied1Aluminum cup, 2 oz1Burner fuel1Burner stand1Digital scale1Glass beaker, 100mL1Graduated cylinder, 25mL1Magnet bar1Metal bolt1Pair of gloves1Pair of safety goggles1Rubber bulb1Ruler1Serological pipet, 2 mL1Short stem pipet1String, 1 m1Thermometer1Volumetric flask, 25.00 mLProcedurePart 1: Length MeasurementsGather the metric ruler, CD or DVD, key, spoon, and fork.Look at the calibration marks on your ruler to determine the degree of uncertainty and number of significant figures that can be made when measuring objects with the ruler.Note: Record every measurement you make with this ruler to the same decimal place. Remember to do this any time you use this ruler throughout the experiment.Measure the length of each of the following objects (CD or DVD, Key, Spoon, Fork) with the ruler in centimeters (cm) to the correct level of precision and record in Data Table 1.Convert the measurements for each of the objects from centimeters to millimeters and record in Data Table 1.Convert the measurements for each of the objects from millimeters to meters and record in Data Table 1.Part 2: Temperature MeasurementsGather the 100 mL glass beaker, cup (plastic or drinking), matches or lighter, burner stand, burner fuel, thermometer, 2 oz. aluminum cup, and aluminum pie pan.Note: The thermometer is shipped in a protective cardboard tube, labeled "thermometer."Look at the calibration marks on the thermometer to determine the degree of uncertainty and number of significant figures that can be made when measuring temperature.Note: Record every measurement you make with this thermometer to the same decimal place. Remember to do this any time you use this measuring device throughout the experiment.Turn on the tap water to hot. Let the water run as hot as possible for approximately 15 seconds.Fill the 100 mL glass beaker with approximately 75 mL of hot tap water.Measure the temperature of the hot tap water with the thermometer in degrees Celsius (°C) to the correct precision of the thermometer. Record the measurement in Data Table 2.Note: When measuring the temperatures place the thermometer into the water so that the silver bulb is fully submerged, but not touching the sides or bottom of the glass beaker. The measurement is complete when the thermometer remains the same temperature without changing.Put on safety glasses.Assemble the burner setup and light the fuel, as shown in Figure 14.Place an aluminum pie plate on a solid work surface away from flammable objects.Set the burner stand towards the back of the pie plate.Place the beaker on the center of the stand. Uncap the burner fuel and set cap aside. Place the burner fuel on the pie plate just in front of the stand.Use matches or a lighter to ignite the fuel. BE CAREFUL- the flame may be nearly invisible. Gently slide the fuel under the stand without disturbing the beaker. The small, 2 oz. aluminum cup will be placed over the fuel to extinguish the flame. Set the aluminum cup next to the burner setup so you are ready to extinguish the flame at any point.Note: When the burner is lit, the flame may be barely visible.Figure 14. Burner fuel setup.Allow the water to heat unit it comes to a full boil. As soon as the water is boiling fully, measure the temperature with the thermometer in degrees Celsius (°C), to the correct level of precision. Record the measurement in Data Table 2.Allow the water to continue boiling for approximately 5 minutes. After 5 minutes, measure the temperature with the thermometer in degrees Celsius (°C) to to the correct level of precision. Record the measurement in Data Table 2.Use the small, 2 oz. aluminum cup to extinguish the burner fuel flame. See Figure 15.Do not touch the metal stand or the beaker; they may be hot.Carefully slide the burner fuel canister out from underneath the burner stand. The sides of the burner fuel canister will be warm, but not hot.Place the aluminum cup directly over the flame to smother it. The cup should rest on top of the fuel canister, with little or no smoke escaping. Do not disturb the burner stand and beaker; allow everything to cool completely.Once all equipment is completely cool, remove the aluminum cup and place the plastic cap back on the fuel. Ensure that the plastic cap “snaps” into place to prevent fuel leakage and evaporation. The aluminum cup, fuel, and all other materials may be used in future experiments. Figure 15. Using the aluminum cup to extinguish the flame.Allow the 100 mL beaker to cool before touching it.Turn on the tap water to cold. Let the water run as cold as possible for approximately 15 seconds..Fill the cup (plastic or drinking) approximately half-full with cold tap water.Measure the temperature of the cold tap water with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Add a handful of ice cubes to the cup of cold tap water and allow them to sit in the cold water for approximately 1 minute.After 1 minute stir the ice water with the thermometer.Measure the temperature of the ice water after 1 minute with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Allow the ice to remain in the water for an additional 4 minutes.After the additional 4 minutes stir the ice water with the thermometer.Measure the temperature of the ice water after 4 minutes with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Convert the temperature measurements for each of the 6 water samples from °C to °F and K. Record the converted temperatures in Data Table 2.Part 3: Mass MeasurementsGather the pen or pencil, 5 pennies, 3 quarters, 4 dimes, and the key.Read the instructions on how to use the digital scale. The lid of the scale must be opened to expose its weighing surface and make mass measurements.Note: There may be a cardboard protector between the scale base and top. If so, remove the cardboard from the scale.Turn the scale on by pressing the Φ/T button.Make sure the scale is reading in grams by looking for the letter "g" in the upper right corner of the scale, if the "g" is not showing then press the "M" button until the scale is reading in grams.Review the different object(s) listed in Data Table 3.Estimate the masses for each of the object(s) in grams and record in Data Table 3. To help you with this process, a penny has a mass of approximately 2.5 grams.Tare the scale by pressing the Φ/T button so that the scale reads 0.0 g.Place the pen or pencil on the scale to measure the mass of the object. Record the mass in Data Table 3 under “Actual Mass (g).”Repeat steps 33 and 34 for the remaining object(s) in Data Table 3.For each object(s), convert the actual mass (in grams) to kilograms (kg). Record in Data Table 3.
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Riverside City College Chemistry Writing and Balancing Chemical Equations Exercises
writing ionic equations :1.Classify each of the compounds as a molecule or a salt.Molecule SaltAnswer bank :CaS, NO2, C2H5 ...
Riverside City College Chemistry Writing and Balancing Chemical Equations Exercises
writing ionic equations :1.Classify each of the compounds as a molecule or a salt.Molecule SaltAnswer bank :CaS, NO2, C2H5OH,KI,C6H6,CaSO42.Classify each of the ions as a cation or an anion.Cations AnionsAnswer bank : NO-/2, K+, Co3+,NH+4, Br-, OH-,SA2+,CO-/3, Ca2+, O2-3.Classify each of the ions as monoatomic or polyatomic.Monoatomic ions Polyatomic ionsAnswer bank : NO-2, OH-,Cu+, Be2+,S2-, H3O+, Sn2+, Na+,F-,O2/2-, CIO-/34.Balance the equations by inserting coefficients as needed.equation 1:PCl3+Cl2⟶PCl5equation 2:Mg3N2+HCl⟶MgCl2+NH35.Balance each equation by inserting coefficients as needed.equation 1:KHF2⟶KF+H2+F2equation 2:P4O10+H2O⟶H3PO46.Balance the chemical equation by adding coefficients as needed.equation: NaOH(aq)+NaNO2(aq)+Al(s)+H2O(l)⟶NH3(aq)+NaAlO2(aq)7.Write the formula for an ionic compound formed from the K+ ion and each additional ion.K+ and Cl− :K+ and N3− :K+ and S2− :8.Write the formula for an ionic compound formed from O2− with each of the ions.magnesium ion:sodium ion:aluminum ion:9.Predict the formula for a compound made from X2+ and Y2−.Insert subscripts as needed.formula: XY10.Give the formula for an ionic compound formed from each pair of ions.Na+ and O2−Al3+ and F−Mg2+ and S2−Ca2+ and P3−11.Determine the formula unit for the compound formed when each pairs of ions interact. Li+ and O2−:Mg2+ and S2−:Al3+ and Cl−:Na+ and N3−:12.Write the chemical formula for the compound formed by each pair of positive and negative ions.Ba2+ and NO3−:Al3+ and CO32−:K+ and PO43−: 13.Write the net ionic equation, including phases, that corresponds to the reactionZn(NO3)2(aq)+Na2S(aq)⟶ZnS(s)+2NaNO3(aq)net ionic equation:14.Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) and KCl(aq). Refer to the solubility rules as needed.net ionic equation:15.Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states.A. copper(II) sulfate, CuSO4, and potassium hydroxide, KOHnet ionic equation:B. lithium carbonate, Li2CO3, and aluminum nitrate, Al(NO3)3net ionic equation:C. sodium phosphate, Na3PO4, and barium chloride, BaCl2net ionic equation:17.Complete and balance the molecular equation for the reaction of aqueous iron(III) nitrate, Fe(NO3)3, and aqueous lithium hydroxide, LiOH. Include physical states.molecular equation:Fe(NO3)3(aq)+LiOH(aq)⟶Enter the balanced net ionic equation for the reaction. Include physical states.net ionic equation:18.Complete and balance the molecular equation for the reaction of aqueous sodium sulfate, Na2SO4, and aqueous barium nitrate, Ba(NO3)2. Include physical states.molecular equation:Na2SO4(aq)+Ba(NO3)2(aq)⟶Enter the balanced net ionic equation for this reaction. Include physical states.net ionic equation:19.Complete and balance the molecular equation for the reaction of aqueous sodium carbonate, Na2CO3, and aqueous nickel(II) chloride, NiCl2. Include physical states.molecular equation:Na2CO3(aq)+NiCl2(aq)⟶Enter the balanced net ionic equation for this reaction. Include physical states. net ionic equation:20.At temperatures above roughly 800 °C, calcium carbonate decomposes. Write and balance the equation for this reaction. Phase symbols are optional.21. For the chemical reaction2HBr(aq)+Ba(OH)2(aq)⟶2H2O(l)+BaBr2(aq)write the net ionic equation, including the phases.net ionic equation:22.Write the net ionic equation for the chemical reaction shown. Include physical states.HClO2(aq)+NaOH(aq)⟶H2O(l)+NaClO2(aq)net ionic equation:23.For the chemical reactionHClO4(aq)+NaOH(aq)⟶H2O(l)+NaClO4(aq)write the net ionic equation, including the phases.net ionic equation:Which ions are considered spectator ions for this reaction? H+ClO−4Na+OH−24.Complete and balance the equation for this single-displacement reaction. Phases are optional.equation:AgNO3+Al⟶25.Complete and balance the equation for the single-displacement reaction. Phases are optional.equation:Li+NaOH⟶26.Consider the decomposition reaction ? ⟶CaO(s)+CO2(g)
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20200927140105lab 7 Groundwater Worksheet
Save this document to your computer, fill in the information, and submit it via Canvas. Note that the worksheet will not b ...
20200927140105lab 7 Groundwater Worksheet
Save this document to your computer, fill in the information, and submit it via Canvas. Note that the worksheet will not be accepted for credit if the ...
University of Florida Drug Controlled Substance Hypothesis Statistical Lab Report
1. Write a Quality Assurance guide for the analysis of one of the following samples; both samples are suspected of having ...
University of Florida Drug Controlled Substance Hypothesis Statistical Lab Report
1. Write a Quality Assurance guide for the analysis of one of the following samples; both samples are suspected of having a drug, but have not undergone any testing as of yet:• A bag containing 100 grams of white powder suspected to contain a controlled substance (drug)OR100ml of human urine suspected to contain a controlled substance (drug)Please remember to address the following topics: scope, Terminology, Testing Facility, Personnel, QA Manual Documentation, Evidence Control, Chemical Reagents, Presumptive testing and confirmatory analytical Procedures, Validation, Equipment Maintenance and Calibration, Proficiency Testing, Audits, Deficiency of Analysis/Corrective Actions, and Health and Safety.Depending upon the analysis being performed, some items may not be applicable whereas other components may need to be added. Also, remember that you can reference a number of standard procedures (SOPs) by referring to established SOPs – you do not need to provide the specifics of the analysis but rather just an overview of the best practice to analyze the sample – which includes optimization of available resources such as analytical instruments and personnel. (20 points)The following FBI quality assurance guidelines summarize the essential goals and are helpful as a reference for this module as well as for the assignment:http://www.fbi.gov/about-us/lab/forensic-science-communications/fsc/jan2005/standards/2005standards15.htm (Links to an external site.)2. This following project involves the testing and comparison of quantitative results produced by two labs using two different analytical methods. A final report will need to be created following the completion of this project. Project Scenario: Two individual laboratories (Lab A and Lab B) were contracted to analyze 25 blood samples to determine the concentration of cocaine (and/or any metabolites) in each sample. Both labs used instrumentation that provided quantitative results, but each lab used a different method. Lab A utilized liquid chromatography- mass spectrometry (LCMS) and Lab B utilized gas chromatography-mass spectrometry (GCMS). For this project, each laboratory was tasked with analyzing the blood samples of 25 known cocaine users. As this project involved the comparison of Lab A with Lab B’s final results, each lab needed to analyze the same 25 samples. As these labs were located in different cities, two tubes of blood were drawn from each of the 25 subjects. One blood tube was sent to Lab A and the second was sent to Lab B so that each lab would have the same 25 samples to compare. Now that the testing has been completed, a final report needs to be created to address whether or not the results from the two laboratories are equivalent.For this assignment, you will need to write a brief outline for this project’s final report. This report should follow a clear structure and include all of the required components as described in the module’s reading. Be sure that the report you submit includes information on the two labs, the two different methods used, and 25 fictitious concentration results per lab. Additionally, be certain to include and explain all of the components that would be required for this final report as discussed in the reading. The concentration data must be included and a statistical analysis of that data must be included as a part of this report. Please consider the following when completing this assignment:* What does your fictional cocaine concentration data look like? You need to come up with your own fictional data for this assignment (the values for the concentrations should be in units of ng/mL). You must include the 25 concentration results for each lab as a part of the data as well as the results of the calculated statistics. You can simply present this concentration data in an Excel table or chart format* The statistical comparison needs to be calculated using either a student t-test or Wilcoxon. You must perform the statistical analysis on your fictional data and compare Lab A to Lab B. You must also provide a conclusion as to whether or not the two methods were comparable.Useful links:Cocaine analysis in various body fluids: https://www.researchgate.net/publication/14750172_Cocaine_and_benzoylecgonine_in_saliva_serum_and_urine (Links to an external site.)Research report guidelines: http://www.nlm.nih.gov/services/research_report_guide.html (Links to an external site.) You may also have to refresh some knowledge of statistical testing since you will be comparing two groups. Here is some reading material:“An Introduction to Statistics”, Driscoll P, Lecky F, Crosby M, J Accid Emerg Med, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725369/ (Links to an external site.)“An Introduction to hypothesis testing. Parametric comparison of two groups-1”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725552/ (Links to an external site.)“An Introduction to hypothesis testing. Parametric comparison of two groups-2”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725593/ (Links to an external site.) “An Introduction to hypothesis testing. Non-Parametric comparison of two groups-1”, Driscoll P, Lecky F, Emerg Med J, 2001, http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1725625/
4 pages
Bio Part 3
Directions for the students: There are 4 essay questions. Please be sure to complete all of them with thorough substantive ...
Bio Part 3
Directions for the students: There are 4 essay questions. Please be sure to complete all of them with thorough substantive responses. Citations are ...
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Lab Worksheet Module08
Use the Wave on a String Simulation for this lab. For this first simulation, click Pulse on the top left, and the rulers a ...
Lab Worksheet Module08
Use the Wave on a String Simulation for this lab. For this first simulation, click Pulse on the top left, and the rulers and timer on the bottom ...
Moraine Valley Community College Length Temperature and Mass Lab Report
Complete lab and fill out document attched with it.1Aluminum pie pan1Bottle of distilled water1Box of matches or lighter1D ...
Moraine Valley Community College Length Temperature and Mass Lab Report
Complete lab and fill out document attched with it.1Aluminum pie pan1Bottle of distilled water1Box of matches or lighter1DVD or CD4Dime1Fork1Isopropyl (rubbing) alcohol (C3H8O), 91%1Key1Pair of scissors1Pen or pencil5Penny1Plastic cup3Quarter1Sheet of white paper1Source of ice cubes1Source of tap water1Spoon1White granulated sugar (C12H22O11)HOL Supplied1Aluminum cup, 2 oz1Burner fuel1Burner stand1Digital scale1Glass beaker, 100mL1Graduated cylinder, 25mL1Magnet bar1Metal bolt1Pair of gloves1Pair of safety goggles1Rubber bulb1Ruler1Serological pipet, 2 mL1Short stem pipet1String, 1 m1Thermometer1Volumetric flask, 25.00 mLProcedurePart 1: Length MeasurementsGather the metric ruler, CD or DVD, key, spoon, and fork.Look at the calibration marks on your ruler to determine the degree of uncertainty and number of significant figures that can be made when measuring objects with the ruler.Note: Record every measurement you make with this ruler to the same decimal place. Remember to do this any time you use this ruler throughout the experiment.Measure the length of each of the following objects (CD or DVD, Key, Spoon, Fork) with the ruler in centimeters (cm) to the correct level of precision and record in Data Table 1.Convert the measurements for each of the objects from centimeters to millimeters and record in Data Table 1.Convert the measurements for each of the objects from millimeters to meters and record in Data Table 1.Part 2: Temperature MeasurementsGather the 100 mL glass beaker, cup (plastic or drinking), matches or lighter, burner stand, burner fuel, thermometer, 2 oz. aluminum cup, and aluminum pie pan.Note: The thermometer is shipped in a protective cardboard tube, labeled "thermometer."Look at the calibration marks on the thermometer to determine the degree of uncertainty and number of significant figures that can be made when measuring temperature.Note: Record every measurement you make with this thermometer to the same decimal place. Remember to do this any time you use this measuring device throughout the experiment.Turn on the tap water to hot. Let the water run as hot as possible for approximately 15 seconds.Fill the 100 mL glass beaker with approximately 75 mL of hot tap water.Measure the temperature of the hot tap water with the thermometer in degrees Celsius (°C) to the correct precision of the thermometer. Record the measurement in Data Table 2.Note: When measuring the temperatures place the thermometer into the water so that the silver bulb is fully submerged, but not touching the sides or bottom of the glass beaker. The measurement is complete when the thermometer remains the same temperature without changing.Put on safety glasses.Assemble the burner setup and light the fuel, as shown in Figure 14.Place an aluminum pie plate on a solid work surface away from flammable objects.Set the burner stand towards the back of the pie plate.Place the beaker on the center of the stand. Uncap the burner fuel and set cap aside. Place the burner fuel on the pie plate just in front of the stand.Use matches or a lighter to ignite the fuel. BE CAREFUL- the flame may be nearly invisible. Gently slide the fuel under the stand without disturbing the beaker. The small, 2 oz. aluminum cup will be placed over the fuel to extinguish the flame. Set the aluminum cup next to the burner setup so you are ready to extinguish the flame at any point.Note: When the burner is lit, the flame may be barely visible.Figure 14. Burner fuel setup.Allow the water to heat unit it comes to a full boil. As soon as the water is boiling fully, measure the temperature with the thermometer in degrees Celsius (°C), to the correct level of precision. Record the measurement in Data Table 2.Allow the water to continue boiling for approximately 5 minutes. After 5 minutes, measure the temperature with the thermometer in degrees Celsius (°C) to to the correct level of precision. Record the measurement in Data Table 2.Use the small, 2 oz. aluminum cup to extinguish the burner fuel flame. See Figure 15.Do not touch the metal stand or the beaker; they may be hot.Carefully slide the burner fuel canister out from underneath the burner stand. The sides of the burner fuel canister will be warm, but not hot.Place the aluminum cup directly over the flame to smother it. The cup should rest on top of the fuel canister, with little or no smoke escaping. Do not disturb the burner stand and beaker; allow everything to cool completely.Once all equipment is completely cool, remove the aluminum cup and place the plastic cap back on the fuel. Ensure that the plastic cap “snaps” into place to prevent fuel leakage and evaporation. The aluminum cup, fuel, and all other materials may be used in future experiments. Figure 15. Using the aluminum cup to extinguish the flame.Allow the 100 mL beaker to cool before touching it.Turn on the tap water to cold. Let the water run as cold as possible for approximately 15 seconds..Fill the cup (plastic or drinking) approximately half-full with cold tap water.Measure the temperature of the cold tap water with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Add a handful of ice cubes to the cup of cold tap water and allow them to sit in the cold water for approximately 1 minute.After 1 minute stir the ice water with the thermometer.Measure the temperature of the ice water after 1 minute with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Allow the ice to remain in the water for an additional 4 minutes.After the additional 4 minutes stir the ice water with the thermometer.Measure the temperature of the ice water after 4 minutes with the thermometer in degrees Celsius (°C) to the correct level of precision. Record the measurement in Data Table 2.Convert the temperature measurements for each of the 6 water samples from °C to °F and K. Record the converted temperatures in Data Table 2.Part 3: Mass MeasurementsGather the pen or pencil, 5 pennies, 3 quarters, 4 dimes, and the key.Read the instructions on how to use the digital scale. The lid of the scale must be opened to expose its weighing surface and make mass measurements.Note: There may be a cardboard protector between the scale base and top. If so, remove the cardboard from the scale.Turn the scale on by pressing the Φ/T button.Make sure the scale is reading in grams by looking for the letter "g" in the upper right corner of the scale, if the "g" is not showing then press the "M" button until the scale is reading in grams.Review the different object(s) listed in Data Table 3.Estimate the masses for each of the object(s) in grams and record in Data Table 3. To help you with this process, a penny has a mass of approximately 2.5 grams.Tare the scale by pressing the Φ/T button so that the scale reads 0.0 g.Place the pen or pencil on the scale to measure the mass of the object. Record the mass in Data Table 3 under “Actual Mass (g).”Repeat steps 33 and 34 for the remaining object(s) in Data Table 3.For each object(s), convert the actual mass (in grams) to kilograms (kg). Record in Data Table 3.
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