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lab 5 - H 2(g Using Dalton’s law of partial pressures we...

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Elizabeth Farrington Experiment #5 Discussion The purpose of this lab is to determine the molar volume of a gas. We will learn how to measure the volumes of gases and calculate the molar volume. We will use Dalton’s law of partial pressures. For Part I we measured the amount of oxygen gas formed from hydrogen peroxide 2H 2 O 2(l) →2H 2 O (l) +O 2(g) by setting up an apparatus that displaced water when oxygen gas was formed. We measured the displaced water, did some calculations and found the molar volume to be 23.87n/L. For Part II we found the amount of hydrogen gas using the same apparatus. Mg (s) +2HCl (aq) →MgCl 2(aq)
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Unformatted text preview: +H 2(g) Using Dalton’s law of partial pressures we calculated the molar volume to be 23.7n/L. We learned to correctly use Dalton’s law of partial pressures to find the molar volume of gases. One error could be the hydrogen and oxygen gases dissolving in the water, lowering our displacement measurement. Another error could be a small leak; the gases would then displace less water, lowering our molar volumes. Even though we checked for leaks and couldn’t find one, our molar volumes suggest there was one. There is no solution expect maybe a different stopper would have worked better....
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