Molar Mass of a Gas Lab Report

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Molar Volume of a Gas Lab Report
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Abstract:
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The aim of this lab was to determine the volume of one mole of hydrogen gas at STP (standard temperature and pressure). In the experiment, a magnesium ribbon was placed at the bottom of an eudiometer tube and allowed to react with 2M hydrochloric acid. The volume of hydrochloric displacement was measured and calculations determined the molar volume of hydrogen gas produced inside the eudiometer tube. After performing and taking the average data of two trials, it was concluded that the calculated value of one mole of hydrogen gas at STP was about 22.35 L/mol. Rounding up, it can be concluded that one mole equals 22.4 L/mol, which is the accepted value of the volume one mole of an ideal gas takes up. However, there was a 0.357% error, which could have been due to minor problems such as reading the values on the instruments slightly off. In the end, the experiment demonstrated that one mole of hydrogen gas at STP takes up 22.4 L. -------------------------------------------------

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Introduction:

An ideal gas can be defined as a hypothetical gas whose molecules occupy negligible space and have no interactions, therefore exactly obeying the gas laws. However, most of the gases encountered in the real world are real gases which do not strictly obey ideal gas laws. The purpose of this lab is to find the molar volume of H₂ gas at STP. In this experiment, a known mass of magnesium was reacted with a solution of hydrochloric acid and water in an eudiometer tube. The volume of displacement of the reacted solution would determine the total volume of H₂ gas and water vapor produced from the reaction. After the data is calculated and corrected for the differences in temperature and pressure, the result is the volume of one mole of hydrogen gas at STP.

It was hypothesized that the calculated molar volume of H₂ gas from this experiment would be close to the literature value of 22.43 L/mol, although it would be slightly greater/less than 22.43 L/mol because of possible sources of error due to inaccurate measurements of the H₂ gas. The independent variable is the amount of magnesium used for the reaction, and the dependent variable is the volume of H₂ gas produced. Temperature, pressure, and total volume are assumed to be controlled variables during this experiment. -------------------------------------------------

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Experimental Procedures:...
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