CHEM discussion question
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chem_wk_7_dq2.docxMust be own work and use in text citation and references.
(Part 1): Answer discussion question below 2 full paragraph (4-5 sentences EACH paragraph.
1. What is the ideal gas law? What factors cause gases to deviate from ideal behavior? Give specific examples.
1. The ideal gas law can be explained by the kinetic molecular theory. We define ideal gas as consisting of molecules with negligible volume that are in constant random. The ideal gas law states the relationship between absolute pressure (P), volume (V), and absolute temperature (T) in a theoretical, "ideal" gas. Mathematically, the ideal gas law is: PV = nRT, where P is absolute pressure, V is volume, n is the number of moles of a gas, R is the universal gas constant, and T is temperature. Real gases deviate from the ideal gas law at high pressure and low temperature following kinetic theory postulates 1 and 3. From kinetic theory, we expect these deviations, because real molecules do have volume and intermolecular forces do exist. An example of an ideal gas law could be a hot air balloon. As the gas in the hot air balloon is heated (by fire), the volume of the hot air balloon will increase which allows it to fly.
2. The ideal gas law is the equation PV= nRT, which combines all of the gas laws. The variables being: (P) pressure; (V) volume; (n) number of mole of gas; and (T) temperature, leaving the constant (R) gas constant. The ideal gas law includes all the information contained in Boyle's, Charles"s and Avogardo's laws. And the ideal gas law is most accurate for low to moderate pressures and for temps that are not too low. Volume, temperature and pressure can cause a deviation in the law.
3. The ideal gas law comes from the kinetic theory, and summarizes how a gas reacts under different conditions, such as temperature, volume and pressure. To find the ideal gas law from the kinetic theory, you must first find the pressure by multiplying frequency of collisions by the average force. To find the average force you must know its mass as well as its average speed or momentum. In other words, the larger and faster the molecule, the more it will be shown in the force. The finished equation should be PV=nRT. In order for a gas to be an ideal gas, it must first follow the 5 postulates of the Kinetic Theory. Some factors that would cause non ideal behavior would be increased pressure, causing intermolecular forces to increase within molecules.
