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

The Objective of this lab is to experimentally determine the molar mass of an unknown and volatile liquid.

Extracts from this document...

Introduction

THE RELATIVE MOLECULAR MASS OF VOLATILE LIQUIDS Objective The Objective of this lab is to experimentally determine the molar mass of an unknown and volatile liquid. Equipment * Hot Plate * 200 mL Flat Bottom Flask * 1000 mL Beaker * 600 mL Beaker * Flask Clip * Flask Cap * Cork * Ring Stand * 25 ml Graduated Cylinder * Funnel * Buret Clamp * 5.1 mL of Unknown A * Thermometer Experimental Procedure 1. All essential equipment was obtained from instructor. 2. 5.1 ml of Unknown A liquid was measured in a 25ml volumetric flask. 3. The ring stand was setup and the hot plate was placed on the base of the stand. ...read more.

Middle

8. Initially a cork was used to seal the cap of the flask, but then, owing to new instructions, the use of the cork was abandoned. 9. The beaker was heated on the hot plate until the liquid in the flask evaporated. 10. After the liquid evaporated, the water in the beaker was allowed to boil for an additional 5-8 minutes before the hot plate was turned off. 11. The flask was removed from the beaker and a cork was used to seal the cap. 12. The flask was then lowered into a beaker of cold water and allowed to completely cool. 13. ...read more.

Conclusion

Data Table Measurement Value Mass of flask and stopper 123.56 g Mass of flask, stopper, and condensed vapor 124.4 g Temperature of boiling water bath 98.8�C Barometric pressure 740 mm Hg Calculations Measurement Value Pressure of vapor, P 0.9736842105 atm Volume of flask (volume of vapor), V 0.2866 L Gas Constant, R 0.0821 L atm/(mole K) Temperature of vapor, T 371.95�K Mass of vapor, g 0.84 g Number of moles of vapor, n 0.0091383249 M Molar mass of unknown 91.92056661 g Conclusion The expected molar mass of the given liquid was 88g but the molar mass obtained through the experimentation was 91.92056661 g. This discrepancy is most probably a result of mechanical errors such as inaccurate mass provided by the weighing scales, incorrect pressure provided by barometer or inaccurate results of calculations provided by our calculator. ...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. The purpose of this experiment was to determine the molar mass of carbon dioxide ...

    Steps 2, 3 and 4 were repeated until there was no further change in the mass (i.e. the carbon dioxide had displaced all the air in the flask). 6. Thereafter, the flask was filled with water before being sealed, using an excess amount of water to ensure that it was completely filled.

  2. Determining the Molar Mass of Volatile Liquid

    - 1 x Precision Digital Barometer(range: 0~1100mbar abs, �1 mbar) - 1 x Precision-Digital Thermometer (range: -70�C~ +199.9 ?0.1�C) - 1x 5 cm3 Pipette ? 0.015 cm3 - 1x Cartridge Burner - Tripod with wire gauze - Boiling stones - Aluminium foil - Ice water bath Chemicals: - Water - Volatile Liquid Procedure 1)

  1. MOLECULAR WEIGHT OF A VOLATILE LIQUID-Lab report

    Percentage uncertainty of the mass Uncertainty: �0.01g Mass: 0.80g Percentage uncertainty = 1.25% The percentage uncertainty of the molar mass would then be of 2.05%.

  2. Butane Molar Mass Lab

    *Final Volume of Water (mL +/- 0.1mL) Ambient room Pressure (inHg +/-0.02 inHg) Ambient Water Temperature (�C +/- 0.1�C) Water pressure at 22.5�C +/- 0.1�C (mmHg) Trial 1 21.630 21.600 36.0 49.4 30.02 22.5 20.45 Trial 2 21.600 21.560 52.5 66.8 30.02 22.5 20.45 Trial 3 21.550 21.520 57.2 73.0 30.02 22.5 20.45 *Volumes were taken from

  1. Aim: To find the molar mass of butane, by finding the number of moles ...

    * The level of water in the trough rose slightly during the experiment. Data Presentation Graph 1 Analysis of Graph RMM = 53.946 RMMmax = 86.420 RMMmin = 37.037 Percentage uncertainty of RMM: i) (RMMmax - RMM) = 32.474 ii)

  2. Using Solubility Rules to Indentify Unknown Solutions

    Data Collection and Processing: Photograph of Lap Setup: Qualitative Observations and Raw Data Table: Five drops ionic solution � 1/2 drop Five drops ionic solution � 1/2 drop KCl MgCl2 Na2SO4 NaOH BaCl2 MgSO4 KCl NR NR NR NR NR MgCl2 NR Ppt - off white, thick consistency, vapor observed

  1. The aim of our experiment was to find out the molar mass of the ...

    X 100 6.941 1 % deviation = 60% Conclusion: The aim of our experiment was to find out the molar mass of the lithium sample and compare the molar mass to the actual molar mass of lithium from the periodic table.

  2. To determine the molecular mass of an unknown alkali metal carbonate, X2CO3.

    Room temperature - All trials were performed in more or less, the same conditions. APPARATUS AND CHEMICALS: Quantity × Item Purpose 1 x 100 cm3 beaker To hold 0.1M HCl before pouring into burette. 1x 50cm3 burette (±0.05cm3) To ensure volume of HCl used can be determined precisely since a burette is a precise instrument.

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