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# Determination of the relative atomic mass of lithium.

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Introduction

Assessed Practical 3 (AS) Determination of the relative atomic mass of lithium. Method Section 1 Apparatus > Conical Flask > Bowl > Measuring cylinder > Clamp stand > Rubber tubing Procedure I set up the apparatus. Then I carried out the correct measurements of water and lithium. I weighed the lithium as well, however when I did this I removed as much of the oil as possible, but not all of it. This was then placed in a small container. The container with the lithium inside was then placed in a conical flask, upright. A bung was placed on top to ensure the collection of gas was successful. I shook the conical flask so the container fell on its side to allow the reaction to take place. The gas produced was collected in a measuring cylinder. ...read more.

Middle

Lithium reacts with water violently, creating a highly flammable gas Hydrogen. When the lithium reacts with water it also forming lithium hydroxide solution, which is corrosive. Lithium metal also burns in air. So therefore when using the metal lithium take great care, as you will need to wear goggles. Lithium is stored in oil, so when removing the oil wear rubber gloves to stop the metal reacting with any excess water on the skin. Hydrochloric acid is corrosive, so careful use is needed as well as wearing goggles. Results Section 1 It is assumed that 1 mole of gas occupies 24000cm3 at room temperature and pressure: 2Li (s) + 2H2O (l) 2LiOH (aq) + H2 (g) Mass of lithium: 0.135g Amount of hydrogen gas collected: 222cm3 Calculate the number of moles of H2: Deduce the number of moles of lithium: Relative atomic mass of lithium: Section 2 Titration results: Titration Volume of HCl (cm3) ...read more.

Conclusion

However I believe there are a few errors which affect the accuracy of my result. When removing the oil from the lithium you cannot remove all of it, this could effect the weight of the lithium. If you could remove all of the oil this would increase the accuracy of the results. Another error was that the experiment was not fully carried out under standard conditions of 100kPa and 298K. To gain more accuracy I could have measured the pressure and temperature. Another error was that the tubing used was slightly permeable, which meant that H2 could escape to lower the volume of gas collected. To prevent this you could use a non-permeable tube, which would increase the accuracy of the results. ...read more.

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