lab report #1

lab report #1 - Magnesium Oxide has escaped while the lid...

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Mariah Rason April 28, 2010 Chemistry 1M Determination of the Empirical Formula of Magnesium Oxide Abstract A 0.3g of Magnesium Ribbon was heated in a crucible and by calculating the mass before and after the reaction the empirical formula was able to be determined as MgO. The theoretical and actual yield was calculated as 0.52403g of MgO and 0.5191g of MgO respectively. Results Mass Calculations Empty Crucible 18.5534 g Crucible w/ Mg 18.8580 g Crucible w/ Product 19.0715 g Magnesium 0.305 g Product (Oxide) 0.5191 g Oxygen 0.2135 g Theoretical Yield: 0.52403 g of MgO Percent by Mass: O:40% Mg: 60% Percent Yield: 99.06% Discussion The theoretical and actual yield were not the same so the calculations were off just a little bit. This could have been from lifting the top off the crucible during the reaction to check if the Magnesium had burned all the way. The fact that the product was a powdery formal and smelled burnt nail polish remover is evidence that the reaction occurred. If
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Unformatted text preview: Magnesium Oxide has escaped while the lid was lifted, or escaped through the crack then the mass percent calculation would be too low because the weight would not have been exact. If the Magnesium Ribbon had a thin oxide coating prior to the reaction the mass percent would be too high because the mass of the Mg would be calculated as too high. If .3g of Zn was heated instead of Mg the product would have been about the same mass. Possibly heating the Magnesium longer would ensure that all the Magnesium would react completely with all the O2. The results were pretty close to the actual value so the experiment seemed to have been pretty successful. Review Questions 1) See Discussion 2) See Discussion 3) See Discussion 4) See Discussion 5) See Discussion Sample Calculations Metal Used .305 g Product (Oxide) .5191 g Oxygen .2135 g...
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lab report #1 - Magnesium Oxide has escaped while the lid...

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