Determining the mass of calcium carbonate obtained Essay

PurposeThe purpose of the taste was to investigate the mass of atomic number 20 change obtained from the reaction between calcium chloride and atomic number 11 carbonate.Apparatus Three beakers (250 ml) Spatula Balance 0.1g Filtration setup Filter piece Stirring rod Plastic dry wash bottleMaterials Sodium Carbonate Calcium chloride Distilled waterProcedure1. Weigh reveal 4.0g of calcium chloride (111g/mol) and dissolve in enough distilled water.2. Weigh out 6.0g of sodium carbonate (106g/mol) and dissolve in enough distilled water.3. Pour the sodium carbonate solution into the beaker containing calcium chloride solution.4. Stir the mixture. Set up the filtration apparatus. Weigh the drip paper and then filter the mixture. Rinse the beaker and empty the contents in the funnel. Wash the precipitate with distilled water several times.5. Place the filter paper with the precipitate and get off it to dry out. After it is completely dry, then weigh the dry filter paper with the p recipitate.Data Table Measurements taken in the experiment lot of the filter paper2.00g 0.01gMass of filter paper with the precipitate (after filter paper dried)5.10g 0.01gMass of precipitate3.10g 0.01g**The mass has an demerit of (0.01) because of the reading in the mass, in which they take up to only 2 decimal points1. The compare of the reaction that took place is shown below, in which a grey/white precipitate of calcium carbonate was produced.CaCl2 (aq) + Na2CO3 (aq) Ca (CO3) (s) + 2NaCl (aq)Calcium + sodium calcium + sodiumChloride carbonate carbonate chloride2. The abstractive mass and the experimental mass are going to be found out in order to see how much calcium carbonate should be obtained theoretically and how much was produced in the real reaction.To find the theoretical mass of calcium carbonate, firstly we welcome to find the limiting reagent in the reaction.The groyne ratio from the equation isCaCl2 Na2CO31 1The actual mole ratio of reagents present isMass i n g 4 6Molar mass in g mol -1 110.98 105.99n = mass 0.03604 0.056609 . Molar massHaving looked at the mole ratio, it is apparent that since calcium chloride has the lowest number of moles present, it is therefore the limiting reagent.The limiting reagent calcium chloride is therefore used to calculate the theoretical mass of calcium carbonate that can be obtainedTheoretical yield = number of moles of limiting reagent x mass of calcium . carbonate= 0.03604 x (40.08 + 12.01 + 16 + 16 + 16)= 0.03604 x 100.09= 3.6g3. therefrom theoretically the mass of the calcium carbonate that can be obtained is 3.6g. The theoretical yield assumes that everything reacts perfectly, and we are able to recover everything 100%. These ideal conditions are rarely present and so we would expect the actual yield to be less than the theoretical yield for this reason.To calculate the experimental mass, the following calculation is done experimental mass = Mass of filter paper with the precipitate Mass of filter paper= 5.1g 2g = 3.1gAs expected the experimental mass is lower than the theoretical mass.4. It is non advisable to use sodium carbonate to calculate the amount of product in the reaction. The theoretical yield depends on the limiting reagent and non the other. Here the 2 reactants are in a molar ratio 11 but the actual molar ratio is 0.036040.056609. The sodium carbonate is in excess. It is not possible even under ideal conditions for every sodium carbonate to react to form the product. Therefore it is not advisable to use this.ConclusionHaving looked at the results, it is clearly seen that the actual experimental mass is less than the theoretical mass yield. This is not an unexpected result. According to my results the actual mass of the precipitate produced was 3.1g, while that of the theoretical mass is 3.6g. The percentage yield of this reaction can be calculated byPercentage yield = Actual mass X 100 = 3.1 X 100 = 86% . Theoretical mass 3.6The maximal yield of a chemical reaction would be 100%, a value that is never reached. Yields close 90% are called very good, yields above about 75% are called good, yields below about 60% are called modest, whilst yields below 30% are called poor. This experiment had a border-line very good yield in regards to these literature guidelines.In practise the theoretical yield based on the balanced chemical equation is never achieved owing to impurities in reagents, side reactions and other sources of experimental error.The possible sources of error in this experiment whitethorn include Material used may have been tampered with and so would affect the overall results. Wrong measurements were taken. Error arrising from human judgement. The balance only recorded 2decimal points. The filter paper may not have been left long enough to dry.A possible modification to this experiment would be to make the sodium carbonate the limiting reageant rather then the calcium chloride as it was in this case. This would be don e so that we would have a smaller number of moles of sodium carbonate then calcium chloride.Although my experiment was successful, some improvement could have been made to both my experiment and too the experiment. This includes Repeating the measurements for more trials so that more accurate answers could be found. Using an accurate rule to measure the mass, so as to reduce the errors in the experiment. Make sure that none of the compound is accidentally spilled out. Use larger quantities so to reduce the error in their recording