Part of The Student Room Group

  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

The purpose of this lab experiment is to determine whether different ionic compounds containing sodium in ethanol will affect its evaporation rate

Extracts from this document...

Introduction

Lucia Serra IB SL Chemistry Mr. McKeen March 12th, 2012 The Rate of Evaporation of Ethanol With Different Ionic Compounds Dissolved In It Purpose: The purpose of this lab experiment is to determine whether different ionic compounds containing sodium in ethanol will affect its evaporation rate, and if so, how great the difference is (percent) and be able to deduce why the change occurs. They are sodium-containing compounds because they were the most familiar to table salt, have the same number of valence electrons and the results should be fairly close to each other. Variables: * Independent: the different ionic compounds in the ethanol solution * Dependent: The rate of evaporation of ethanol solution * Controlled: * Same ethanol used * Same gas pressure sensor used throughout the entire experiment * Same balance used to measure the mass * 0.3 g of each of the ionic compounds in every trial * Same Erlenmeyer flask used during the evaporation * 10.0 mL of ethanol used in every trial Hypothesis: The ethanol solution with NaF would have the lowest evaporation rate because the interparticle forces between the NaF and C2H6O would be extremely polar because of the hydrogen bonds due to the fluorine in the ionic ...read more.

Middle

NaCl 10.0 mL 0.3 g 1. NaF 10.0 mL 0.3 g 2. NaF 10.0 mL 0.3 g 3. NaF 10.0 mL 0.3 g 4. NaF 10.0 mL 0.3 g 5. NaF 10.0 mL 0.3 g 1. NaI 10.0 mL 0.3 g 2. NaI 10.0 mL 0.3 g 3. NaI 10.0 mL 0.3 g 4. NaI 10.0 mL 0.3 g 5. NaI 10.0 mL 0.3 g *Uncertainty calculated collecting data for 200 seconds with the probe in the classroom and then subtracting the range and diving by two: **Uncertainty calculated by diving the smallest unit (1.0 mL) by two ***Uncertainty calculated by precision of instrument, only measure mass to the tenths place Data Analysis and Processing: Rate of Evaporation (? 0.055 kPa/s) of Different Ethanol Solutions Solution Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 C2H6O 0.001890 0.001555 -0.0004033 -0.0001292 -0.001599 C2H6O + NaF 0.005720 0.003746 0.002062 0.005972 0.001445 C2H6O + NaCl 0.0002420 0.004792 0.0009713 0.001206 0.001038 C2H6O + NaI 0.001903 0.001936 0.003351 0.003207 0.002856 Average Rate of Evaporation: * Mean = sum of trials/ # of trials o Uncertainty= (highest trial - lowest trial) / 2 1. C2H6O: [0.001890 kPa/s +0.001555 kPa/s +(-0.0004033 kPa/s)+(-0.0001292 kPa/s) + (-0.001599 kPa/s)] / 5= 0.0002627 kPa/s a. ...read more.

Conclusion

Also, with the help of another person, less time would be lost between pouring the ethanol into the Erlenmeyer flask and getting everything ready before collecting the data, because a couple of seconds passed by before the button was pressed. A good way to control the time so that the trials in each solution were done around approximate times was to have the mass measured out before starting out the experiment so as to be more efficient; another positive thing was that the controlled variables were kept constant throughout the experiment. Something that would help in the future would be to hold more trials, because we can see that with five, proportionately, the difference in some of the trials within each series were very different, and having more reproducible results would give more stable averages. Also, in a more advanced course, creating a vacuum would ensure that there are no other particles in the Erlenmeyer flask besides the ethanol and the solution and also having the same temperature. This is because gases in the air affect the pressure and if they reacted with any of the substances, then it would alter the pressure that the gas pressure sensor collects. ?? ?? ?? ?? Serra ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

or


Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Ionic and Molecular Compounds Lab

    Unknown 2 could also be an acid since it had a pH level of 4, which is fairly acidic. Unknowns 3 and 6 could be ionic compounds because they were neutral and conducted electricity. Unknowns 8 and 9 could be acids since they both had a high acidity.

  2. Reactivity series for common metals experiment.

    � Lead: No texture/surface/color change (No Reaction) I. Iron Chloride(Fe Cl) with: � Copper: No texture/surface/color change (No Reaction) � Iron: No texture/surface/color change (No Reaction) � Magnesium:Its surface turns black (Reaction � Zinc:Turns black on its surface (Reaction) � Lead: No texture/surface/color change (No Reaction) I. Magnesium Sulphate(MgSO4)with: � Copper: No texture/surface/color change (No Reaction)

  1. Change of Potential Difference in Voltaic Cells Lab Report

    This scatter graph represents the potential difference in Voltaic Cells using five different concentrations of copper sulfate solutions throughout the experiment. The scatter and line graphs represent the change in potential difference throughout the experiment using different copper sulfate concentrations.

  2. rate of evaporation

    Water bath machine 1 - Measuring cylinder 3 5 ml Dropper 3 - Stopwatch 3 - Table 1: list of apparatus and material used METHOD 1. Prepare the water bath machine at the temperature of 60.00C 2. Then, prepare a 1ml of 0.1M HCl in an evaporating dish, using a measuring cylinder.

  1. Chemistry Laboratory Report --- Evaporation: Intermolecular Attractions

    Explanation * From Table 1, we can see that non-polar liquids tend to have a greater temperature difference, indicating that it cool down faster, than polar chemicals. This can be explained by the intermolecular forces of the molecules. Non-polar molecules have weaker intermolecular forces, with only van der Waals'

  2. Potassium Iodide Lab

    Data: a) mass of filter papers: b) mass of lead iodide: 3rd period 4th period 1:9 2:8 3:7 4:6 5:5 6:4 7:3 8:2 9:1 c) molar mass of KI: 165.998 g/mol d) molar mass of Pb(NO2)3: 331.268 g/mol e) calculation for determining molarity for each solution based on 1,000 ml: 200 ml/1000 ml x .5 ml = .1 ml f)

  1. The aim of this experiment is to examine the enthalpy of combustion of the ...

    Pentan-1-ol has the greatest number of carbon atoms in the chain and also the highest enthalpy change of combustion. Therefore as the number of carbon atoms increases the enthalpy change also increases. This is because as the number of carbon atoms in a chain increases the number of bonds which can be broken also increases.

  2. Reaction Rate

    Four different concentrations will be trialed- 0.5M, 1.0M, 1.5M and 2.0M- each three times and then averaged out so that we achieve a more accurate result. We will alter this variable by changing the concentration of the H2SO4 solution in order to determine a relationship between the strength of

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work