Determination of the Molar Volume of a Gas and the Universal Gas Constant
DETERMINATION OF THE MOLAR VOLUME OF A GAS
AND THE UNIVERSAL GAS CONSTANT
Salve, Ryan Angelo TAB3, Group 6, Mr. John Kevin Paulo Biadomang Tabor, Frances Hermilyn March 8, 2013

I. Abstract
This experiment is working with the ideal gas law, which is the summation of Boyle’s Law, where pressure is inversely proportional to volume, Charles’ Law, where the volume is directly proportional to temperature and Avogadro’s Law, where the volume is directly proportional to moles. In this experiment, the volume occupied by one mole of H2 was determined. By measuring the volume of H2 gas generated, its molar volume can also be calculated. The universal gas constant can be …show more content…
V. Results The results of the experiment were shown below.
Table 2 Atmospheric Pressure  760 mm Hg  Atmospheric Pressure in kPa  101.308 kPa  Temperature of H2O in beaker  28°C  Temperature in Kelvin  301.15 K  Vapor Pressure measured at indicated temperature  3.77239 kPa  Corrected Pressure of gas in cylinder  97.53561 kPa 
Table 3. Results of the trials  Trial 1  Trial 2  Trial 3  Average  Volume of gas (L)  0.0056  0.0064  0.0062  0.0061  Length of Mg ribbon reacted (cm)  0.4  0.4  0.4  0.4  Mass of Mg ribbon reacted (g)  0.0057  0.0062  0.0056  0.0058  Moles of Mg used (mol)  2.34 x 104  2.55 x 104  2.30 x 104  2.39 x 104  Moles of H2 produced (mol)  2.34 x 104  2.55 x 104  2.30 x 104  2.39 x 104  Ratio of volume of gas generated to moles of gas produced, V/n  23.93 L/mol  25.10 L/mol  26.96 L/mol  25.33 L/mol  Universal gas constant (kPaV/nT)  7.75 kPa∙Lmol∙K  8.08 kPa∙Lmol∙K  8.73 kPa∙Lmol∙K  8.19 kPa∙Lmol∙K 
VI. Discussion To determine the pressure of H2 in the cylinder, the vapour pressure of the water was subtracted from the atmospheric pressure. This formula was derived from Dalton’s Law of partial pressure, Ptotal=Pgas+PH2O
The partial pressure of water vapour depends on the temperature of the water bath. To obtain the partial…

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