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

Heat combustion of Alcohol

Extracts from this document...

Introduction

High Level Chemistry Heat of combustion of alcohol Design Prac Student: Kathy Nguyen Teacher: Mr Underwood Due Date: 23rd May 2009 To investigate the effect of one factor on the heat of combustion of the alcohol Background Information Alcohols are used as a source of fuel in many countries. For it to turn into fuel, alcohol must be burnt. Alcohol is also a good clean source of energy and heat. In this experiment I will be trying to find out the amount of energy produced when different alcohols are burned. In this experiment, the type of alcohol will be tested is Ethanol. Ethanol is a colourless liquid and is sometimes referred simply as alcohol or spirits. Carbon chains with a hydroxide molecule at the end of the chain make up an alcohol. Ethanol is a straight-chain alcohol and its molecular formula is C2H5OH. Its empirical formula however is C2H6O The heat of combustion of any substance is the amount of heat energy given out when 1 mole of that substance burns completely in air. ...read more.

Middle

Avoid contamination and residue to the next experiment when using the thermometer Distilled water will be used to thoroughly clean out the equipments before experiment. Equipments will not be reused for the next experiments. Materials * 3 L of water * 200 mL of 0.5 Molar ethanol in beaker * 200 mL of 1.0 Molar ethanol in beaker * 200 mL of 1.5 Molar ethanol in beaker * 200 mL of 2.0 Molar ethanol in beaker * 200 mL of 2.5 Molar ethanol in beaker * Bottle containing 800 mL of Distilled water * 15 � 150 mL Conical flask * 1 � Metal clamp * 1 � Wooden tongs * 1 � Retort stand * 15 � Spirit burner * 1 � Thermometer (� 0.01 �C) * 1 � Match box * 1 � Electronic scale (� 0.02 g) * 1 � Permanent pen * 5 � Label stickers Method Drawing up data tables Molar of Ethanol Trials Initial temp (�C) Final temp (�C) Temp change (�C) Initial mass (g) ...read more.

Conclusion

Weigh the spirit burner attached with the lid containing the alcohol and record the initial mass 8. Place the spirit burner under the conical flask and use the matched to light the wick 9. When the water temperature reaches approximately 40�C, blow out and extinguish the flame 10. Record the exact temperature reached when flames were extinguished 11. Using the tongs, move the spirit burner and lid to the electronic scale and weigh the final mass 12. Dispose the water and alcohol inside the spirit burner 13. Repeat steps 1 - 11, but change the type of ethanol in respect to independent variables 1.0 Molar, 1.5 Molar, 2.0 Molar and 2.5 Molar of ethanol 14. When repeating steps 1 - 11, make sure a new conical flask and water is used and also a new spirit burner is used 15. When all five experiments of the different molar concentration of ethanol is completed, repeat the experiment another two times for each molar concentration of ethanol in reference to the data table Calculations 1. Final temp - Initial temp = Temp change (�C) 2. Final mass - Initial mass = Mass used (g) ?? ?? ?? ?? Mr Underwood HL Chemistry Design Prac Kathy Nguyen Page 2 of 6 ...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. Molar Heat combustion chemistry - investigate the effect of molar mass on the molar ...

    and light the burner. 8. Gently stir the water with the thermometer and when the temperature has risen by 20oC, extinguish the burner by carefully replacing the cap. 9. Continue stirring for 10 seconds, then read and record the final water temperature.

  2. Determining the effect of carbon chain length of an alcohol on its fuel efficiency

    Heat the water until it reaches 300C. * Extinguish the spirit burner by placing it's stopper on top the wick and keep stirring the water and note down the highest temperature it reaches. * Re-weigh the spirit burner and record the mass of alcohol that has been burned.

  1. Chemistry extended essay - investigate the effect of 2-bromo-2-methyl propane concentration and temperature of ...

    5- Using a graduated cylinder measure 67 ml of distilled water added to an Erlenmeyer flask #4. 6- Add two drops of Bromo-phenol blue indicator to flask #4. A, a, II:- 1- Add quickly the solution in Erlenmeyer flask #4 to solution in flask #3 and start the stop watch to count for time in seconds.

  2. Enthalpy of Combustion of Alcohols Lab

    Volume of water used * Distance between beaker and flame Materials 100 cm3 Methanol 100 cm3 Ethanol 100 cm3 Butan-1-ol Distilled or De-ionized water Calorimeter Tripod Electronic Balance 100 cm3 Graduated Cylinder Retort Stand 50 cm3 Conical Flask Cotton Aluminum Paper Gas Click Lighter Stopwatch Thermometer Stirring Rod Clamp Hot

  1. Determination of Heat of Combustion of Ethanol

    uncertainty for ΔH = 2.55 + 1.10 = 3.65% % uncertainty to absolute uncertainty of ΔH = 3.65*833.92/100 = 30.43 KJ/mol Absolute uncertainty of ΔH = -833.92 ±30.43 KJ/mol Trial 2 Moles of Ethanol = 1.90/46.08 Moles of Ethanol = 0.0412 ±0.0004 mol

  2. Bomb calorimetry. The goal of this experiment was to use temperature data over ...

    -4983.1522 kJ mol-1 However, ± 2% is the accuracy on the fairly simple apparatus used, hence, âcUonapthalene and âcHonapthalene in this combustion are âcUonapthalene = -4982.66 ± 99.6532 kJ mol-1 âcHonapthalene = -4983.1522 ± 99.6630 kJ mol-1 Enthalpies of formation of naphthalene From the eq.(15), Theoretical Enthalpies of formation of naphthalene using Hess’s Law is âfHonapthalene = (10x(-393kJ/mol)+4x(-285kJ/mol))

  1. Analysis of the Standard Enthalpy of Combustion for Alcohols

    Different liquids could result in a difference in the strength of attractive forces between particles, meaning a different specific heat capacity which would affect the calculation of energy gain to water using the equation q=mcâT, and thus an incorrect enthalpy change value.

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

    Calculate the average temperatures for every alcohol that has been used in the previous experimental process. 2. Use graphing techniques to represent your results. 3. Calculate the heat given out to the known sample of water in the boiling tube.

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