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

relative atomic mass of lithium

Extracts from this document...


Determination of the Relative Atomic Mass of Lithium To find out the relative atomic mass of lithium I am going to use two methods. In Method 1 I will use the volume of hydrogen produced as lithium reacts with water. In method 2 I will titrate the lithium hydroxide which is the solution formed from my first experiment. METHOD 1 Table of results Mass of Lithium used (g) 0.08 Initial volume of water in measuring cylinder (cm3) 320 Final volume of water in measuring cylinder (cm3) 148 Volume of hydrogen gas produced (cm3) 172 Treatment of results The equation below shows lithium reacting with water in method 1. 2Li(s) + 2H2O(l) 2LiOH(aq) + H2(g) This equation will help me deduce the number of moles used. The following formula can be used to determine the number of moles of hydrogen gas produced. No of moles = volume 24000 No of moles of hydrogen = 172cm3 24000 = 0.00716 moles Looking at the equation it shows that for every 2 moles of lithium reacted, 1 mole of hydrogen is produced. This means the number of moles of hydrogen must be multiplied by 2 in order to find the number of moles of lithium. No of moles of lithium = 0.00716 x 2 = 0.01432 moles = 0.0143 moles (3 significant figures) Now that I have figured out the number of moles of lithium, I can work out the relative atomic mass of lithium by using the following formula:- Relative atomic mass ...read more.


(Do not put back into jar because this will contaminate the whole chemical) Hydrochloric acid can be corrosive and cause burns. However the Hydrochloric acid being used in the experiment is diluted so it's not corrosive. 4. If some hydrochloric acid or distilled water is split on the floor, clear it up very quickly to prevent other people slipping over it and getting injured. 5. When putting hydrochloric acid into the burette, use a filter to prevent any spillages and therefore stop people slipping over it. Make sure you are not standing on a chair whilst pouring hydrochloric acid down the filter. If you cannot reach the filter, than use a sink instead of a table to pour the chemical into the burette. 6. Handle phenylethene with care by wearing gloves because it can be irritating to eyes and skin. EVALUATION As I did my experiment there were errors made. Firstly as I carried out method 1, it was difficult to remove all the oil from the lithium. Some oil may have stayed on the lithium during the experiment and caused error. To overcome this error I could use a tissue to wipe off all the oil on the lithium. If the lithium gets darker around the edges, than the edges can be chopped up in order to keep the lithium fresh. Also a non-polar solvent can be used to make sure there is no oil left on the lithium. ...read more.


This piece of equipment is easier to use and is more reliable because it doesn't allow any gas to escape and has a higher level of accuracy when taking down readings. On the other hand the measuring cylinder is harder to use due to it being used under a water bath and so the hydrogen gas is more likely to escape as it travels through the rubber tube into the measuring cylinder. I think the titration method was more accurate than the collecting hydrogen gas method. This is because when I was collecting my hydrogen gas, it was difficult for me to keep the conical flask in an upright position and therefore some gas may have escaped even if I had moved just a little bit. Also the gas that was produced when lithium had reacted with water was passed through rubber tubes. Some gas may have stayed in the tubes after the reaction had stopped causing error and unreliable results. On the other hand when I was carrying out my titration I had used a burette which didn't let any hydrochloric acid escape. However this method wasn't totally accurate due to the number of iodine drops added could have been to heavy or too light and the concentration of hydrochloric acid added to the lithium hydroxide using the burette could have been slightly too much. In conclude there were many areas for error in both methods (slightly more in method 1) but other than that the experiment was successful. ?? ?? ?? ?? Sachin Patel 12TU4 Mr Wright ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic 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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    The fourth figure I recorded from my burette isn't a real significant figure as it could only be a 0 or a 5. My rough titrations were used to see the approximate volume of acid needed to neutralise the sodium carbonate.

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    We are going to use a 250cm3 one in order to ensure we have enough solution for the whole titration. * Pasteur pipette A Pasteur pipette is small enough to allow us to add very small quantities of solvent. We use it to add the last centimetre before reaching the graduation mark of the volumetric flask.

  1. Peer reviewed

    Investigation to determine the Relative atomic mass of Li

    5 star(s)

    1 : 1 From reacting ratios no. of moles of LiOH is equal to the number of moles of HCl. - No. moles of LiOH = 0.004235 mol Calculate the number of moles of Li: Using the equation: 2Li (s) + 2H2O (l) --> H2 (g) + 2LiOH (aq)

  2. effects Concentration and Temperature on the Rate of Reaction

    However, this time use a heating plate rather than a magnetic stirrer so that temperature can be adjusted. 2. Mix 5cm3 of potassium bromate(V) solution, 5cm3 of sulphuric acid solution and 5cm3 of phenol solution in a boiling tube and add 4 drops of methyl orange indicator.

  1. Lab report Determination of Enthalpy Change of Neutralization

    + H2O (l) CH3COO- (aq) + H+ (aq) Therefore, a part of energy from neutralization has lost tp push the reaction towards the right side. It results in the enthalpy change of neutralization of ethanoic acid is smaller than that of the strong acid. H2S (aq) + H2O (l)

  2. Finding Out how much Acid there is in a Solution

    * Balance: * Volumetric Flask (250cm3): * Pipette (25cm3): * Burette: From this, I can calculate that the total percentage error for the equipment of my investigation is 1.06%. The effect of this on my final value for the acid concentration is given by the percentage of the final value that this percentage corresponds to.

  1. The Chemistry oh Phosphorous

    In addition to this, phosphorus is essential for all human activity. Every chemical reaction that happens within every cell in a living organism requires energy. From such processes that occur continuously (eg. the metabolism) to specific needs (eg. muscle contraction), a store of energy is required.

  2. The Effects of Strong and Weak Acids on the Order of a Reaction.

    Using one of each will confuse the experiment at I would then be measuring two different things, rather than the one I intend to do. I will therefore be using Hydrochloric Acid (HCl)

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