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Determination of the molar mass of magnesium

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Kamil KamiÅski IB2 02/12-12 Determination of the molar mass of magnesium Introduction: This experiment will be an attempt to determine the molar mass of magnesium. For that we will have an experiment where we dissolve sulphur into hydrochloric acid. Then we measure the amount of gas created during the reaction. To get the molar mass itself we will have to make sure to record the conditions of the experiment such as the temperature or pressure. Material: The material used for the experiment was: 1. eudiometer 2. thermometer 3. barometer 4. measuring cylinder (1000 cm3) 5. Stand with clamp 6. magnesium ribbon 7. hydrochloric acid Method: 1. About 20mm of magnesium ribbon and weight it with the accuracy of 0.001g 2. Pour 5cm3 of HCl into the eudiometer. ...read more.


Result: Before the experiment the magnesium was carefully weighted on a scale. After turning the eudiometer the HCl started to go down towards the magnesium through the water. Once it reached it a reaction took place creating bubbles of air that went up to the top and pushed the water level down. Once the reaction ended all the magnesium was gone. During the reaction the temperature was read of a thermometer and the pressure of a barometer to get the most accurate values. finally we measured the volume of air inside the eudiometer. Table 1: Data type Result Unit weight of magnesium 0.033 g ±0.001 temperature 24 C ±0.5 pressure 753 mmHg ± 0.5 volume of gas inside the eudiometer after the reaction 34.6 ml ± 0.05 Percentage uncertainty: Data processing: The equation for molar mass looks like this: Changing the temperature to Kelvin: Gas constant (R) ...read more.


Then I would like to put extra attention on the thermometer and especially the barometer. The thermometer could only show whole degrees which is a great loss to precision. Then the barometer seemed quite old and unstable and the need to convert the pressure to Pascal and finally reading from it was quite hard which in my opinion was altogether quite hard. Also these where only the conditions in the entire room. One cannot be sure if they where exactly the same in the tube. Especially the temperature of water could have been quite different. Then of course the amount mg could have impossibly been measured accurately and we can't be sure if exactly all of it reacted. Also the unknown pureness of the reactants and the solvent could justify the error in the result. My suggestions for improvements is to begin with is use of more precise instruments. Then a different method involving a more closed environment and a different method for gathering data. ...read more.

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