Determining the mass of calcium carbonate obtained Essay

PurposeThe purpose of the sample was to investigate the kitty of atomic number 20 change obtained from the reaction between calcium chloride and sodium carbonate. in like mannerl Three beakers (250 ml) Spatula Balance 0.1g Filtration setup Filter written report Stirring rod cell Plastic wash bottleMaterials Sodium Carbonate Calcium chloride Distilled body of waterProcedure1. Weigh out 4.0g of calcium chloride (111g/mol) and dissolve in comme il faut distilled water.2. Weigh out 6.0g of sodium carbonate (106g/mol) and dissolve in sufficient distilled water.3. Pour the sodium carbonate solution into the beaker containing calcium chloride solution.4. Stir the mixture. exercise up the filtration apparatus. Weigh the filter paper and then filter the mixture. rinse off the beaker and empty the contents in the funnel. Wash the come with distilled water some(prenominal) times.5. Place the filter paper with the precipitate and leave it to dry out. by and by it is completely d ry, then weigh the dry filter paper with the precipitate. entropy Table Measurements taken in the prove bulk 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 book has an error of (0.01) because of the reading in the smokestack, in which they showing up to lone(prenominal) 2 decimal points1. The equation of the reaction that took tail end is shown downstairs, 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 divinatory mass and the experimental mass argon going to be found out in order to see how much calcium carbonate should be obtained notionally and how much was produced in the real reaction.To buzz off the theoretical mass of calcium carbonate, firstly we have to find the hold in reagent in the reaction.The mole ratio from t he equation isCaCl2 Na2CO31 1The demonstrable mole ratio of reagents present isMass in 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 wherefore the limiting reagent.The limiting reagent calcium chloride is therefore used to calculate the theoretical mass of calcium carbonate that canful be obtainedTheoretical progeny = number of moles of limiting reagent x mass of calcium . carbonate= 0.03604 x (40.08 + 12.01 + 16 + 16 + 16)= 0.03604 x c.09= 3.6g3. hence theoretically the mass of the calcium carbonate that can be obtained is 3.6g. The theoretical beget 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 followi ng computation is doneExperimental 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 not the other. Here the two reactants are in a mill ratio 11 but the actual molar ratio is 0.036040.056609. The sodium carbonate is in excess. It is not possible nevertheless under ideal conditions for every sodium carbonate to react to take a hop the product. Therefore it is not advisable to use this.ConclusionHaving looked at the results, it is clear 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 careful 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 rank that is never reached. Yields just about 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 establish 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 may 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 hand long enough to dry.A possible modification to this experiment would be to make the so dium carbonate the limiting reageant rather then the calcium chloride as it was in this case. This would be done so that we would have a smaller number of moles of sodium carbonate then calcium chloride.Although my experiment was successful, many 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. victimisation an accurate method 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