Good Example of a poor Lab report

Sayed Ahmed Lab report Lab results Mass of the Crucible and lid Mas of crucible, lid, and MgSO4.nH2O Mass of crucible, lid and MgSO4 Data Collected 22.7g 26.2g 24.5g Data Analysis The mass of water (H2O) released is 1.7g. The result was obtained through the measure of magnesium sulphate (MgSO4) 3.5g, and after the evaporation, it was measured again and was 1.8, but the weight boat adds extra weight which is considered and uncertainty. The scale was rising above the zero by 0.2 and it is considered as an uncertainty. Equation (3.5g ± 0.6g) – (1.8 ± 0.2g) 1.7g ± 0.8g To find the actual amount of H2O evaporated; subtract 0.8 from 1.7 and the actual result would occur to 0.9g of water evaporated. This result is proved to be correct in the table above. 22.7g is the mass of crucible and lid, and the mass of them combined with MgSO4.nH2O is 26.2g. 3.5g + 22.7g = 26.2g To calculate the uncertainty the equation would lead to (3.5g ± 0.6) + (22.7g ± 0.2g) 26.5g ± 0.8g Calculating moles The mole of Magnesium Sulphate (MgSO4) present is 0.014 mol. Use the mass of the experiment and divide it by the atomic mass of MgSO4 120.36x = 1.8g X = 1.8 ÷ 120.36 X = 0.014 mol The mole of water (H2O) released is 0.094g. Use the mass of the experimented H2O released and divide it by the atomic mass of H2O. 18x = 1.7 X= 1.7 ÷ 18 X= 0.094g Find the mole ratio of MgSO4 to H2O 18.02X= 1.8g X= 1.8÷18.02 X= 0.1 Divide 0.014 by 0.1 X= 0.1÷0.014 X= 7 (actual number 7.14) The ratio is 7:0.1 Conclusion The formula to the hydrate of MgSO4 or Magnesium Sulphate is MgSO4 ? 7H2O = 7MgSO4 ± 7H2O Alternate Conclusion Magnesium Sulphate turns into a powder due to the lack of Water (H2O), but as soon as it reacts with the water evaporated in the atmosphere, it slowly changes to its original form (MgSO4 ? nH2O)