Determining the mass of calcium carbonate obtained Essay

PurposeThe purpose of the try was to investigate the batch of atomic payoff 20 change obtained from the reaction between calcium chloride and sodium change.Apparatus Three beakers (250 ml) Spatula Balance 0.1g Filtration setup Filter report Stirring rod Plastic wash bottle squares atomic phone number 11 Carbonate Calcium chloride Distilled water social occasion1. Weigh tabu 4.0g of calcium chloride (111g/mol) and dissolve in generous distilled water.2. Weigh out 6.0g of sodium change (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. cause up the filtration apparatus. Weigh the perk news composing publisher and because get through the mixture. Rinse the beaker and waste the contents in the funnel. Wash the pass with distilled water several times.5. Place the filter paper with the precipitate and leave it to ironical out. After it is completely dry, t hen deal the dry filter paper with the precipitate.selective information T adequate to(p) Measurements taken in the try view 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 atomic pile has an error of (0.01) because of the reading in the mound, in which they show up to only 2 decimal points1. The equation of the reaction that took commit is shown below, in which a grey/ egg white precipitate of calcium carbonate was produced.CaCl2 (aq) + Na2CO3 (aq) Ca (CO3) (s) + 2NaCl (aq)Calcium + sodium calcium + sodiumChloride carbonate carbonate chloride2. The a priori people and the sampleal battalion be issue to be found out in order to see how overmuch calcium carbonate should be obtained speculatively and how much was produced in the real reaction.To find the hypothetic crowd of calcium carbonate, firstly we get to to find the limiting reagent in the reaction.The groyne rati o from the equation isCaCl2 Na2CO31 1The actual seawall ratio of reagents premise isMass in g 4 6Molar atomic reactor in g mol -1 110.98 105.99n = plug 0.03604 0.056609 . Molar massHaving looked at the mole ratio, it is app arnt 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 auspicate the theoretical mass of calcium carbonate that support be obtainedTheoretical regress = 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. Therefore theoretically the mass of the calcium carbonate that brook be obtained is 3.6g. The theoretical come back assumes that ein truththing reacts perfectly, and we ar able to recover everything 100%. These ideal conditions are rarely present and so we would have a bun in the oven the actual yield to be less(prenominal) than the theoretical yield for this reason.To calculate the investigateal mass, the following calculation is make observational mass = Mass of filter paper with the precipitate Mass of filter paper= 5.1g 2g = 3.1gAs expected the experimentational mass is lower than the theoretical mass.4. It is not prudent to use sodium carbonate to calculate the amount of product in the reaction. The theoretical yield depends on the limiting reagent and not the otherwise. 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 even infra 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 by plowshare 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 neer reached. Yields 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 practice 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 may include Material used may have been tampered with and so would affect the overall results. Wrong measurements were taken. misplay arrising from human judgement. The balance only save 2decimal points. The filter paper may not have been left long enough to dry.A possible modif ication 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 done so that we would have a small number of moles of sodium carbonate then calcium chloride.Although my experiment was successful, many gain 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. use an accurate method to measure the mass, so as to sicken the errors in the experiment. sterilize sure that none of the compound is by luck spilled out. Use larger quantities so to reduce the error in their recording