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Lab report - Determine the Empirical Formula of Magnesium Oxide by reacting a known mass of Magnesium with Oxygen.

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__________ Grade 11 Lab report Chemistry Lab report ? Empirical Formula of Magnesium Oxide Determine the Empirical Formula of Magnesium Oxide by reacting a known mass of Magnesium with Oxygen. Safety Risk Assessment: Properly follow lab safety guidelines by wearing lab coats, gloves, and goggles and clear any personal belongings off the experiment area or the apparatus table. Gently handle glassware. Be careful when dealing with Bunsen burners. Make sure the crucible does not break while heating it as it might break due to the immense air pressure inside. ...read more.


0.01875(±100%)/0.01875(±100%) =1(±200%) Whole number ratio 10(±4g) 3(±6g) Empirical Formula: Mg10O3 Evaluation Error Significance Improvement Using an inaccurate weight balance. We used a balance that is to the tenths only High We should have used a balance correct to the hundredths. Opened lid. We lost some smoke that was fine Magnesium oxide. Medium We should have used a steel funnel, which would allow oxygen to enter but prevent gaseous products from escaping. Incomplete combustion. Magnesium did not burn completely. High We should have carried out with a better supply of oxygen, or heat it for longer period of time. ...read more.


Therefore we see were nowhere close obtaining a empirical formula to the theoretical answer though according to our uncertainty for Oxygen which is ±3 it could be the oxygen we had weighed 5g and so therefore giving us a much accurate result of Mg10O2 which would go to a simplest ratio of Mg2O which would be closer to the theoretical answer. In addition to this according to our huge uncertainty the ratio could have also been 1:1 if the ratio would have led to 6:6. Though we see that the reason behind getting such an inaccurate answer is due to the incomplete combustion and due to not using a much more precise and accurate balance to weigh the apparatus and chemicals used. ...read more.

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