# Stp Lab

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The problem of the experiment was to determine the volume of one mole of H_(2(g)) at STP. In a way, the problem is essential in understanding how one mole of an ideal gas at STP is always equivalent to 22.4 L. By determining if the volume of a mole of H_(2(g)) is 22.4 L, it supports Avogadro’s law that one mole of an ideal gas occupies 22.4 L at STP. At the same time, it indicates that a direct relationship exists between volume and the number of moles of gas as temperature and pressure stays constant. One real world application of the importance of this problem is demonstrated when a helium balloon is lighter than an identical balloon filled with air (http://antoine.frostburg.edu/chem/senese/101/gases/faq/everyday-gas-laws.shtml).
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The experimental value for the volume of one mole of H_(2(g)) at STP was approximately 29.1 L, but the predicted result was 22.4 L. By calculating (29.1 L)/(22.4 L) * 100, the percent error was 30%, which indicates that there was a source of scientific error. The experimental design itself may have also contributed to a source of error because in order for Avogadro’s law to apply the concept that a mole of a gas occupies 22.4 L at STP, H_(2(g)) must have been treated as an ideal gas. Therefore, with the room temperature condition of 294.5 K and the barometric pressure of 99.02 kPa inside the lab, it may have caused H_(2(g)) to act as a real gas. In order for a gas to resemble more of an ideal gas, the temperature must be very high and the pressure must be very low. In addition, both the eudiometer and pan was filled with tap water, which may contain other kinds of compounds that may have reacted with the magnesium strip. As a consequence, it is possible that entire magnesium strip did not only react with〖 H〗_(2(g)), but with other compounds included in the tap

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