Chem 151 Gas Behavior
Ideal Gas Behavior
Author: VanessaStoll
Lab Partners: Janelle Vallejo
Instructor: Nieves Montano
Chem 151, Section 002G
Date Work Performed: February 12, 2014
Date Report Submitted: February 20, 2014
Abstract:
This paper reports a lab experiment done on the ideal gas law to determine differences in gas based upon their “R” constant difference to 0.082057. A total of seven gases were tested, which included, Ethanol, Hexane, Cyclohexane, Pentane, Ethyl Acetate, Butane and Acetone. These gases were each heated and then condensed to liquid gas to find specific values and determined Ethanol as the gas closest to ideal behavior in this experiment.
Introduction:
The Ideal Gas Law demonstrates the relationship of the properties of gases. This relationship is specific to the gases that are considered “ideal”. For a gas to be considered “ideal,” it will have no interactions with other molecules and the molecules that make up the gas won’t take up any space.
The Ideal Gas Law equation is PV=nRT. “P” stands for pressure, “V” is for volume, “n” gives the number of moles, “R” is the gas constant and “T” is for temperature. The ideal gas constant value is 0.082057 (L x atm)÷(mol x K). The purpose of the experiment was to be able to measure the temperature and the mass of each gas tested, to configure a constant and determine which gas is the most “ideal”. To configure “R” the equation will be, R= PV ÷ nT.
Based on our knowledge of an ideal gas, we hypothesized Pentane will have the most ideal behavior to real gas and Cyclohexane to be the least ideal. We expect Pentane to be the most ideal because it’s boiling point is the furthest away from the boiling point of water. To test our hypothesis, we used heat to vaporize each gas, an ice bath to cool the gases down and measured the condensed liquid gas to calculate each gas’s constant.
Methods:
In this experiment, we first measured the mass of an empty flask using the balance for our
Author: VanessaStoll
Lab Partners: Janelle Vallejo
Instructor: Nieves Montano
Chem 151, Section 002G
Date Work Performed: February 12, 2014
Date Report Submitted: February 20, 2014
Abstract:
This paper reports a lab experiment done on the ideal gas law to determine differences in gas based upon their “R” constant difference to 0.082057. A total of seven gases were tested, which included, Ethanol, Hexane, Cyclohexane, Pentane, Ethyl Acetate, Butane and Acetone. These gases were each heated and then condensed to liquid gas to find specific values and determined Ethanol as the gas closest to ideal behavior in this experiment.
Introduction:
The Ideal Gas Law demonstrates the relationship of the properties of gases. This relationship is specific to the gases that are considered “ideal”. For a gas to be considered “ideal,” it will have no interactions with other molecules and the molecules that make up the gas won’t take up any space.
The Ideal Gas Law equation is PV=nRT. “P” stands for pressure, “V” is for volume, “n” gives the number of moles, “R” is the gas constant and “T” is for temperature. The ideal gas constant value is 0.082057 (L x atm)÷(mol x K). The purpose of the experiment was to be able to measure the temperature and the mass of each gas tested, to configure a constant and determine which gas is the most “ideal”. To configure “R” the equation will be, R= PV ÷ nT.
Based on our knowledge of an ideal gas, we hypothesized Pentane will have the most ideal behavior to real gas and Cyclohexane to be the least ideal. We expect Pentane to be the most ideal because it’s boiling point is the furthest away from the boiling point of water. To test our hypothesis, we used heat to vaporize each gas, an ice bath to cool the gases down and measured the condensed liquid gas to calculate each gas’s constant.
Methods:
In this experiment, we first measured the mass of an empty flask using the balance for our