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

Chemistry Lab Report: Calculation of the Empirical Formula of Magnesium oxide

Extracts from this document...

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

    To reach molar ratios, the number of moles of magnesium and oxygen were reached and simplified into the lowest whole number ratios. The empirical formula of magnesium oxide was then decided. During data processing, the percentage uncertainties associated with masses were found so that the percentage uncertainties of the number of moles were concluded.

  2. Change of Potential Difference in Voltaic Cells Lab Report

    For 50ml of copper sulfate solution, divide the 1L mass by 20 = = 12.485g of CuSO4.5H2O Dissolve 12.485g of CuSO4.5H2O in 50 ml distilled water, using a volumetric flask. Use the formula: C1V1 = C2V2 to prepare different concentrations of copper sulfate from the stock solution of 1M concentration.

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

    3.Number of moles of magnesium. = 0.0091 Mole (the number of moles of magnesium = mass / atomic weight . the atomic weight of magnesium is 24.3 g / mole ) 4.Number of moles of oxygen atoms that were used.

  2. IB Chemistry - Boyle's Law Lab Report

    From the Boyles' law, P?1/V � P=k(1/V), PV=k(constant) can be deduced. Form the mathematical calculation based on the Boyles' law, the volume was exactly decreased, when the pressure was increased. In addition, Pressure*Volume showed the constancy, even if it contained huge uncertainties. Therefore, the conclusion will be same as Boyles' law that the pressure and the volume are inversely proportional.

  1. Determining the empirical formula of magnesium oxide lab

    Therefore the percent uncertainty for the mass of the magnesium is 20%. 0.2�0.004114=0.000823 This means that the uncertainty for the number of moles in the magnesium is �0.008228mol. These are the calculations for determining the uncertainty of the number of moles of oxygen.

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

    Whichever point the two lines meet at can safely be assumed to be a good estimate of the maximum temperature reached and how much time had elapsed. Graph 1: Highest temperature reached in Part X, Trial 1. For the best estimation of maximum temperature reached, a magnified view of the intersection of horizontal line and y-axis is useful.

  1. Finding the empirical formula of magnesium oxide

    O=16.00gmol-1 Percentage of Mg, x100%=60.31% Percentage of O2, x100%=39.69% R.M.M of MgO= 40.31gmol-1 R.A.M of Mg=24.31gmol-1 R.A.M of O=16.00gmol-1 Percentage of Mg, x100%=60.31% Percentage of O2, x100%=39.69% Percentage of error 2Mg+O2?2MgO element Mg MgO ratio 2 2 Number of moles 0.0123 mol X X=0.0123 mol Theoretical mass of MgO, 0.0123

  2. Finding thr Percentage Composition of Magnesium Oxide

    The water could have been contaminated. Also, the weighing scale could have been faulted. Recommendations Part B of this investigation was lacking and this caused confusion with the procedure. For future classes, Part B should be added. Also, the Apply & Extend questions should be clearer as they were quite confusing.

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