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

Enthalpy of paraffin wax Lab

Extracts from this document...


Chemistry Enthalpy of Paraffin Wax lab Aim: Calculate an experimental value for the enthalpy of Combustion of paraffin wax Variables Independent variable: Amount of heat released by the combustion of paraffin wax Dependant variable: Enthalpy of combustion of paraffin wax Controls: The candle used to release energy must be the same throughout the experiment, to ensure that the wax is the same. This will be done by only using one wax candle The aluminium can used to heat up the water must remain the same so that it's mass does not change due to the carbon molecules on the bottom from the heat and so that no water escapes the system. ...read more.


Measure the temperature of the water in the can and note it down 4. Place the candle below the can (which is suspended above it using a clamp attached to a pole) 5. light the candle 6. Wait around 5 minutes before noting down the temperature of the water 7. blow out the candle and push it aside carefully and swiftly 8. Take the mass of the candle and note it down in your datatable. 9. Weigh the can with the water, take the final mass down and jot down how much water was lost during the procedure 10. Repeat steps 1 to 9 for the second trial Datatable Trial 1 Trial 2 Initial temperature of water (c) ...read more.


Second Experimental Value for enthalpy of combustion (Kj/mol) Theoretical Value for enthalpy of combustion (Kj/mol) -10613.63 -10027.5 -13774 Reasons for difference : Improvements More trials could be done We could time the amount of time the paraffin wax candle burns to give us more even values Water was lost when removing and placing the thermometer, this could be avoided by having the thermometer in the water the whole time, but then the thermometer would absorb the heat as well. Sources of error : Some water and paraffin wax was lost to then environment during the experiment, this can not be changed. Some of the heat was escaping to the atmosphere from the candle, this could not be improved because the candle needs oxygen to burn so we could not place it in an insulated environment. ...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. Enthalpy of Combustion Lab Report

    = 908 - 908 5. (1.31 ? 46.1) = 0.00284 (4.18 ? 6.8 ? 82.3) = 2339 2339 (2339 ? 0.00284) = 823 - 823 Since the combustion of ethanol is an exothermic reaction, the sign of is negative.

  2. Heat of Combustion Lab

    We measured the final temperature to see the changes of the temperature. We blew out the candle when the temperature reaches 35�C, and we measured the highest temperature reached as the final temperature. When the temperature reaches 35�C, we quickly blew out the candle.

  1. Thermodynamics: Enthalpy of Neutralization and Calorimetry

    20.2 �.71 C� e = .0296 e =.0351 1103.448 � .029 gC� 851.834 �????? gC� ( 1.00 cal/gC�)(1103.448 � .0296 gC�)= ( 1.00 cal/gC�)(851.834 �?????1 gC�)+ HC (20.2 �.71 C�) (1103.448 � .0296 cal) = (851.834 �?????1 cal) + HC (20.2 �.71 C�)

  2. Change of Potential Difference in Voltaic Cells Lab Report

    So, the amount of zinc sulfate needed is: 14.377 5= 71.883g Hence, dissolve 71.883g of zinc sulfate in 250 ml distilled water, using 250ml volumetric flask. Preparation of Potassium Chloride (KCl) solution To prepare the salt bridge solution; 250 ml of 1M KCl is needed for the 5 sequences.

  1. Enthalpy of Combustion of Alcohols Lab

    hands PROCEDURE Making an Alcohol Lamp: * Take a 50 cm3 Conical Flask * Take cotton and roll it in your hands to make the wick. * The wick needs to fit snug in the hole and reach to the bottom of the jar.

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

    Incomplete transmission of heat is assumed due to the movements caused in the laboratory, which affected the flame and therefore the transmission. Qualitative data Mass of prpanol Mass 1 Mass 2 Mass 3 Average mass Initial mass g ± 0.01 122.31 145.44 139.81 135.85 Final mass g ± 0.01 120.15

  1. Analysis of the Standard Enthalpy of Combustion for Alcohols

    more heat energy from the surroundings, directly affecting the temperature change and therefore, q=mcâT and the âH value. Distance between the conical flask and alcohol lamp A clamp will be set at a distance of 25 cm from the table, and this the flask will sit at the same height each trial.

  2. The chemistry of atmospheric and water pollution.

    Replace CFCs with compounds which have significantly lower ozone depletion potentials (ODP) such as hyfrochloroflurocarbons (HCFCs). These compounds are effective as they are attacked while in the lower atmosphere thus it does not reach the stratosphere to attack ozone. However these compounds are more expensive and in some cases less effective than CFCs in various applications.

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