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"Properties of Gases"
Properties of Gases
Shelia Olander

The values for the universal gas constant R, and the volume of one mole of gas were determined. The experiment values of R and the volume of one mole of gas were then compared to the accepted values. The experimental values of R obtained were 0.09067 (L∙atm/mol∙K), 0.09514 (L∙atm/mol∙K), and 0.09040 (L∙atm/mol∙K). The molar volumes of hydrogen gas obtained were 0.1306 (L/mol), 0.1365 (L/mol), and 0.1390 (L/mol). The percent error of R was 12.20%, and the percent error of the molar volume was 99.40%.


The purpose of this experiment was to determine the value of the universal gas constant R (L∙atm/mol∙K), and the molar volume of hydrogen gas. In this experiment, a known mass of magnesium reacted with an excess amount of hydrochloric acid to produce hydrogen gas. The reaction that took place in the experiment was as follows:

Mg (s) + 2HCl (aq) MgCl2 (aq) + H2 (g)

The balanced net ionic equation was as follows:

Mg (s) + 2H+ (aq) Mg2+ (aq) + H2 (g)

The value of R was calculated using the Ideal Gas Law (PV = nRT), and the van der Waal's equation (P + an2/V2) (V-nb) = nRT. The value of R should be closer to the R value obtained from van der Waal's equation than the Ideal Gas Law because carbon dioxide was not under ideal conditions. The molar volume of hydrogen gas was determined at a known temperature and pressure. The hydrogen gas was collected in a graduated cylinder by the downward displacement of water. The volume of gas collected was then converted to the volume of pure hydrogen using the Ideal Gas Law.

The experiment was important because it demonstrates the behavior of gases when it is not under ideal conditions, such as high pressures and low temperatures. Understanding the behavior of gases is important in understanding the...

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"Properties of Gases." Sep 24, 2018
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