ucsb - chem 1a - lab 5 discussion

ucsb - chem 1a - lab 5 discussion - (III) chloride (FeCl3)...

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Lab 5: The Molar Volume of Gases – Discussion Lab five consisted of calculating gas at standard temperature and pressure by using the ideal gas law and Dalton’s law. Both parts of the lab started by assembling an apparatus that would measure gas produced. The gas product from the reactants we placed in one flask would travel through a tube connecting to another flask, displacing water that would travel through another tube to a beaker. The water displaced would then be the volume of gas produced. The difference between the two parts lay in the reactants used and what was produced. In part one, oxygen gas (O2) was produced by mixing 20mL of 3% hydrogen peroxide (H2O2) with 4.5mL of three moles iron
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Unformatted text preview: (III) chloride (FeCl3) acting as a catalyst: 2 H2O2 + FeCl3 -> FeCl3 + 2 H2O + O2 In part two, we mixed a strip of magnesium with 4.5mL of 3M HCl: Mg + 2 HCl -> H2 + MgCl2 The calculated molar volumes at STP ended up relatively close to the expected value, off by only a few digits. However, a snag was encountered with the calculations for hydrogen gas. The volume originally measured was 220mL, opposed to the expected estimate of 70mL. Possible explanations for this error lie within the procedure (flasks not equalized; tubes accidentally moved, causing more water displacement)....
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This note was uploaded on 05/19/2008 for the course CHEM 1AL taught by Professor Hooker during the Fall '07 term at UCSB.

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