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

Percent Yield Experiment. The limiting reagent for this experiment is strontium chloride hexahydrate. The two products will be strontium sulphate as a solid and copper (II) chloride in an aqueous state.

Extracts from this document...

Introduction

Percent Yield Lab By Sean Frank SCH3U - 11 University Chemistry Mr. Posteraro November 26th 2012 All Saints High School Hypothesis: The limiting reagent for this experiment is strontium chloride hexahydrate. The two products will be strontium sulphate as a solid and copper (II) chloride in an aqueous state. The predicted precipitate is strontium sulphate and the reaction should precipitate out approximatly 0.65 g of the substance. Materials: 1. 1 100 ml Wash Bottle 2. 2 50 ml Beakers 3. 1.00g Strontium Chloride hexahydrate 4. 1.00g Copper (II) Sulphate pentahydrate 5. 1 Glass Funnel 6. 1 Filter paper (type 2) 7. 1 250ml Erlenmeyer Flask 8. 100ml Water 9. 1 Digital Scale (precsision withtin a hundredth of a gram) 10. 1 Stirring Rod Apparatus: Procedure: 1. Fill the wash bottle with 100 ml of water 2. Using a digital scale, measure 1g of strontium chloride hexahydrate into a 50ml beaker. 3. Repeat step 2 with 1g of copper (II) sulphate pentahydrate 4. Using the control digital scale (teacher's scale), weigh the filter paper and record its weight. 5. Using the wash bottle, add enough water to the beaker containing the 1g of strontium chloride hexahydrate to completly dissolve the solid compound. Avoid adding any more than nessesary. ...read more.

Middle

Therefore there is 0.6888 grams of strontium sulphate Calculation 4: Percent Yeild Given: Mass of strontium sulphate precipitate 0.66 g Theoretical mass of strontium sulphate 0.6888 g Procedure: Yeild = (Experimental mass/theoretical mass) x 100 = 0.9582 x 100 = 95.82 % ? Therefore the percent yeild of strontium sulphate in this experiment is 95.82 % Calculation 3: Percent Error Given: Mass of strontium sulphate precipitate 0.66 g Theoretical mass of strontium sulphate 0.6888 g Procedure: Error = ((Theoretical yeild ? yeild) / theoretical yeild) x 100 = 0.0418 x 100 = 4.18 % ? Therefore the percent error of the strontium sulphate yeild in this experiment is 4.18 % Table 2: Theoretical calculations of the masses and moles of the reactants and products. SrCl2 - 6H20 Cu(II)SO4 - 5H20 SrSO4 Cu(II)Cl2 11H2O 1.00g 1.00g 0.6888g 0.5043g 0.7431g 266.58 g/mol 249.62 g/mol 183.64 g/mol 134.45 g/mol 18.01 g/mol 3.751x103- mol 4.006x103- mol 3.751x103- mol 3.751x103- mol 4.126x102- mol Analysis: 2. The percentage yeild in the experiment is 95.82 %, which is greater than the target yeild of 95 %. The following are possible factors that may contribute to acheiving a higher yeild. Firstly, it is possible that there was contamination from outside sources, such as lint or dust particles that could have fallen into the drying precipitate. ...read more.

Conclusion

First, the ammount of transfers were kept to a minimum in order to preserve as much of the orginal reactants as possible. Multiple transfers can cause reactants or precipitate to adhere to the walls of the beakers or the funnel. There are only two transfers present in this procedure. Second, the solutions were dissolved into aqeous solutions to facilitate a reaction and increase the ammount of reaction taking place. Without a solution, the two substances would not have reacted in a solid state. Solutions also increase the likeliness of the most possible reaction, because of its containment, as opposed to a gas, and the potion of the particles within, unlike a solid. Both reactants were dissolved into water in order to maximise the reaction and ensure it took place. The reaction was finally stirred for a mintute to maximise the reaction. The stirring added heat and motion, which is another form of heat, which allows more reactant to react properly. The heat increases the speed at which the particles move within the liquid, which leads to more collisions, and finally more reaction taking place. Finally, the original beakers and the funnel were washed down with water and passed through the filter to ensure all possible remaining reactant had been added to the apparatus. Refrences: 1. Nelson 11 Chemistry (2005) 2. http://ottawa.ca/en/env_water/water_sewer/water_wells/quality/facts/index.html 3. http://sargentwelch.com/pdf/msds/Strontium_Chloride_6-Hydrate_723.00.pdf 4. https://www.sciencelab.com/msds.php?msdsId=9923597 ...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

    Deducing the quantity of acid in a solution

    5 star(s)

    Having the equipment contaminated can cause inaccuracies in both making the solution and titration because: - Could react with the compounds and ruin the experiment - Could alter the colour of the solution and therefore, alter the endpoint - Could more importantly reduce the concentration All this could affect our results, both numerically and experimentally.

  2. effects Concentration and Temperature on the Rate of Reaction

    This shows that there is again a positive correlation between concentration and reaction rate, as when the concentration of potassium bromide is increased, the reaction rate increases. This means that the reaction, with respect to potassium bromide, is also first order.

  1. Bleaching experiment. Estimation of available chlorine in commercial bleaching solution.

    + 2S2O32-(aq) --> 2I-(aq) +S4O62-(aq)-------------------(3) (1) It is NOT necessary to measure the accurate amount of potassium iodide and ethanoic acid. Why? Both potassium iodide and ethanoic acid act as excess reagent, so that it is not necessary to know the accurate amount, what are the most concerned are that the accurate amount of the limiting reagents.

  2. Making Copper (II) Sulphate Stock Solution evaluation

    to work out the percentage of the concentration that could be incorrect: Percentage Error = Total uncertainty x Concentration 100 = 0.084 x 0.099975961

  1. Extraction of Chlorine

    [3]- http://www.cellchem.com/docs/products-services/chlorine caustic.htm, informative web-site; 27 February. [4]- Extract from: Redox reactions and electrode potentials, Chemical Ideas, Heinemann, page 208. [5]- http://electrochem.cwru.edu/ed/encycl/, electrochemistry encyclopaedia web-site; 28 February. ADVANCED SUBSIDIARY GCE CHEMISTRY (SALTERS) Skills for Chemistry: Open-Book Paper Primary pollutants are formed by oxidation under high temperatures in vehicle engines during

  2. Chemistry - Data Analysis

    Once the graphs were plotted gradients were calculated at temperatures of 80�C, 60�C and 50�C to determine the rate at which the temperature was falling. The results obtained are shown in the table below. Degrees(�C) Polystyrene Cup (Minutes) Plastic Cup (Minutes)

  1. Plan to investigate the transition temperature of salt hydrates

    This is why this force is the weakest [6]. The second force is the: 1. Permanent Dipole ? Permanent Dipole. This force is due to the idea of polar molecules. A polar molecule is a molecule in which there is a difference in electronegativity between the individual atoms and ions.

  2. Testing Nickel (II) Sulphate, Iron (III) Chloride, Potassium Sulphate

    Double replacement reaction is when two ionic reactants break their bonds and associate with the anion or cation which is from other reactant. In the Sodium Hydroxide test; hydroxides occur within the solution once a few drops of sodium hydroxide is added into the solution.

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