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Mass Conservation Essay

1526 words - 6 pages

The conservation of massAIMThe aim of this experiment is to show that mass is conserved during a chemical reaction.The Law of Conservation of Mass, established in 1789 by French Chemist Antoine Lavoisier, states that mass is neither created nor destroyed in any ordinary chemical reaction. Or more simply, the mass of products by a chemical reaction is always equal to the mass of the reactants.The reaction between potassium iodide and lead (II) nitrate under room temperature and atmospheric pressure results with a yellow precipitate. This reaction can be expressed by the equation: 2KI(aq) + Pb(NO3)2(aq) ( PbI2(s) + 2KNO3(aq)HYPOTHESISThe mass before and after a chemical reaction will be the same as mass is conserved.INDEPENDENT VARIABLE:The mass before the reaction(By measuring the mass of the reactants before reaction this independent variable can be controlled)DEPENDENT VARIABLE:The mass after the reaction(By controlling the independent variable this dependent variable can be controlled)CONTROLLED VARIABLES:

Digital balance

Proportion of chemicals


Reaction time






100 mL



Measuring cylinder

25.0 mL



Access to a digital balance




Potassium iodide solution

0.5 mol/dm3

100 mL


Lead (II) nitrate solution

0.5 mol/dm3

100 mL


Glass rod

20 cm



METHODWear safety glasses, apron and covered shoes before setting up any equipment.Measure out 20 mL of potassium iodide with a measuring cylinder and pour into a 100 mL beaker.Measure out 20 mL of lead nitrate with another measuring cylinder and pour into another 100 mL beaker.Zero the balance and put both beakers together on the balance (balance is big enough for two beakers). Weigh their total mass accurately.Record the mass obtained including uncertainties.Carefully pour the lead (II) nitrate solution into the 100 mL beaker containing the potassium iodide.Record the observation during the reaction.Use a glass rod to carefully stir the mixture in order to make sure the reaction is completed. Re-zero the balance. Place both beakers back on balance and weigh their total mass.Record the mass obtained including uncertainties.When finished, pour the contents of the beakers into the laboratory sink.Rinse the beakers and the measuring cylinders under tap water.Dry the beakers and the measuring cylinders.Repeat steps 2-12 another four times to maintain accurate results.Result

Mass before weighing(±0.001g)

Weight after weighing(±0.001g)
















Qualitative data:Yellow precipitate was produced.There were some spillages of the product.Processed data

Mass difference ± 0.002g

Mass difference express as percentage

Random Error





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