Determination of the Molar Volume of a Gas and the Universal Gas Constant
EXPERIMENT NO. 6
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
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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 determined using the ideal gas law. The experiment was done by inverting a graduated cylinder containing HCl and water with the cork assembly that was placed in its mouth into a beaker of ¾ full. The cork assembly was done by using a paper clip with a small piece of Mg ribbon attached to it. Using the equations of gas law, the universal gas constant and the molar volume were calculated. The experiment results lead us into a conclusion that there are possible errors happened during the experiment that made it different from the desired result. II. Keywords: gases, molar volume, gas laws, vapour pressure, partial pressure
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III. Introduction A gas is the state of matter that is characterized by having neither a fixed shape nor a fixed volume. Gases exert pressure, are compressible, have low densities and diffuse rapidly when mixed with other gases. On a molecular level, gases are best described as independent molecules separated by large distances in constant random motion.
Four measurable properties can be used to describe a gas: pressure (P), volume (V), temperature (T) and mole quantity (n). The relationships among these properties are summarized by the Gas Laws.
Table 1. Gas Laws
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 determined using the ideal gas law. The experiment was done by inverting a graduated cylinder containing HCl and water with the cork assembly that was placed in its mouth into a beaker of ¾ full. The cork assembly was done by using a paper clip with a small piece of Mg ribbon attached to it. Using the equations of gas law, the universal gas constant and the molar volume were calculated. The experiment results lead us into a conclusion that there are possible errors happened during the experiment that made it different from the desired result. II. Keywords: gases, molar volume, gas laws, vapour pressure, partial pressure
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III. Introduction A gas is the state of matter that is characterized by having neither a fixed shape nor a fixed volume. Gases exert pressure, are compressible, have low densities and diffuse rapidly when mixed with other gases. On a molecular level, gases are best described as independent molecules separated by large distances in constant random motion.
Four measurable properties can be used to describe a gas: pressure (P), volume (V), temperature (T) and mole quantity (n). The relationships among these properties are summarized by the Gas Laws.
Table 1. Gas Laws