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

Determination of empirical formula lab report

Extracts from this document...

Introduction

SECONDARY SCHOOL DEPARTMENT OF CHEMISTRY Lab report: DETERMINATION OF EMPIRICAL FORMULA Done by: X IB1 November 13, 2008 I. Data Collection and Processing: 1- Data Collection: a) Quantitative Data: Table 1: Masses of material used or produced in the experiment Weighed Material Mass (� 0.001 g) Empty crucible + lid 15.313 Crucible + lid + magnesium before heating 15.336 Crucible + lid + combustion product 15.351 b) Qualitative Data: * At the beginning of the experiment, the magnesium ribbon appeared a silver one-piece thin ribbon. * During the course of heating, the ribbon was transforming gradually into a white/gray product. Moreover, the heating process was attended by ignition of the crucible content and formation of smoke. ...read more.

Middle

= m (MgxOy) - m (Mg) = 0.038 - 0.023 = 0.015 � 0.004 g d. Calculation of the Moles of Oxygen and Magnesium: n (Mg) = m (Mg) � M(Mg) = 0.023 g � 24.31 g.mol-1 = 0.00095 mol (uncertainty to be found in the next question) n (O) = m (O) � M (O) = 0.015 g � 16.00 g.mol-1 = 0.0009 mol (uncertainty to be found in the next question) e. Determination of Uncertainties In Moles: Since the molar mass is a definitional quantity, its uncertainty is zero, thus: ?n (Mg) = 1/24.31 (� 0.002) = � 0.00008 mol ?n (O) = 1/16.00 (� 0.004) ...read more.

Conclusion

2) Evaluating the Procedure: * The Percentage of Purity of Initial Mg: The initial reactant is not 100% pure Mg, otherwise the number of moles of both Mg and O would have been exactly equal, which is not the case. * Side Reactions That Might Have Occurred: * End of the Reaction: After heating the crucible, its lid and the magnesium for almost 10-13 minutes, I noticed that gray powder was no longer forming so I decided that the reaction was over. 3) Improving the Investigation: * The Bunsen Burner was not well functioning so it took us a lot of time to get to the perfect flame. * When the magnesium began to bum, we didn't remove the burner; we kept it until the end of the experiment which we shouldn't have done. ?? ?? ?? ?? ...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

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. Experiment - The Empirical Formula of Magnesium Oxide

    of magnesium and magnesium oxide, i.e., the absolute uncertainty of oxygen = � (0.002 + 0.002) = � 0.004g No. of moles of magnesium, oxygen The formula was employed, MM (Mg) = 24.31g/mol, MM (O) =16.00g/mol, the masses has already been calculated above.

  2. Enthalpy of Combustion Lab Report

    This has been changed for each trial in order to provide more accuracy to the experiment. 3. The mass of the distilled water used in the experimental procedure is an independent variable. This has also been changed for each trial in order to provide a variety of results and cover all aspects of the experimental procedure.

  1. Enthalpy of Combustion of Alcohols Lab

    Moreover, this lab can be further improved by using a calorimeter instead of a beaker. Although the lab design asked to use a calorimeter, due to limited time, we used a beaker instead. A calorimeter is a device used to measure the heat of reaction and as it is insulated,

  2. acid base lab report

    moles = 0.1 M HCl 0.050 L = 0.0050 mol HCl Since our the goal pH is 6 (acidic) acid must be left over. Therefore the volume of NaOH added is unknown (z) Mol NaOH = 0.1 M(z) The total number of final moles of HCl: Mol HCl final =

  1. Lab Experiment : The change in mass when magnesium burns. (Finding the empirical formula ...

    4.Number of moles of oxygen atoms that were used. = 0.0071mole (the number of moles of oxygen = mass / atomic weight . the atomic weight of magnesium is 16.0 g / mole ) 5.Simplest ratio: Mg = 0.0151 Mole = 1.33 0.0135mole Oxygen = 0.0135mole = 1 0.0135mole Multiply by the smallest whole number you can possibly find

  2. IB chemistry revision notes

    May combust incompletely to make C (soot) and CO. * Isomers o Hydrocarbons of the same structural formula, but different structural formulae.

  1. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    Enthalpy of reaction for this trial = ?HY (Trial 1) = 110250J = 110.25kJ.mol-1. For Part Y, Trial 2 Graphical analysis similar to that used in Part Y, Trial 1 has been used to determine the maximum temperature reached in the duration of the reaction.

  2. Discovering the formula of MgO

    5,80 4 0,076 10,864 10,984 0,120 0,044 36,6 8,32 Mass of Product= (Mass of crucible with product)-(Mass of crucible) Uncertainty in mass of product= (Uncertainty in mass of crucible with product) + (Uncertainty in mass of crucible) =0,001+0,001=±0,002 Mass of Oxygen== (Mass of product)-(Mass of magnesium)

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