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Unformatted text preview: of stoichiometry. We found the mass of the reactant Mg to be 0.085g. Since the mole ratio of Mg to H2 is 1:1, moles of hydrogen was equal to moles of magnesium. Dividing 0.085g by 24g (atomic weight of Mg), we found we had 0.0033 mol Mg, which equaled 0.0033 mol H2. Once again, using the same ideal gas law, we determined the volume of hydrogen at STP (V2 = 0.085L (743.523 torr / 762.762 torr) * (294K / 2965K)) to be 0.083L. Dividing 0.083L by 0.0033mol, we found the molar volume of hydrogen to be 25.2 L/mol. The main source of error for this experiment is within the reactions themselves. Hydrogen and oxygen gas most likely partially dissolved in the water, or may have not reacted in the original solution. In both cases, the results would be thrown off, resulting in a lower observed molar volume. Another source of error is caused by equipment accuracy but this is to be expected....
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This note was uploaded on 04/28/2009 for the course CHEM 1AL taught by Professor Hooker during the Fall '07 term at UCSB.
- Fall '07