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gaslaw - 46 Experiment VII Ideal Gas Laws Goals • Study...

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46 Experiment VII: Ideal Gas Laws Goals Study the relationship between pressure and temperature of atmospheric gas at constant volume; Determine the absolute zero temperature in Celsius Study the relationship between pressure and volume at constant temperature Introduction and Background Early studies of gases revealed that in most cases the relationship between pressure, volume, and temperature was essentially independent of the kind of gas involved, as long as the conditions were not close to leading to condensation. Significant advances were made by Boyle, Charles, and Gay- Lassac. Charles discovered that when volume was plotted versus temperature at constant pressure, a straight line resulted, namely, T C V × = . When plots for different gases were compared, they all extrapolated to give zero volume at the same absolute temperature. This is referred to as Charles’ Law. Gay-Lassac studied the relation between pressure and temperature under constant volume and found a linear relationship between the two: T C P × = ' . Again the extrapolation to zero pressure gives the same temperature for different gases. This is now called the Gay-Lassac’s Law. Boyle investigated the relation between pressure and volume at constant temperature and found that . const PV = This is the Boyle’s Law. Combining the results of the three investigators, a universal ideal gas law was derived: nRT PV = , where n is the number of moles and R the ideal gas constant. In this lab we will verify the Gay-Lassac’s law and Boyle law for simple atmospheric gas, and we will use the data for the Gay- Lassac’s experiment to determine the absolute zero temperature on the Celsius scale.

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