1. Out of all the "8" gases [Argon, Hydrogen, Nitrogen, Oxygen, Air, Helium, Methane, Carbon Dioxide], which one is the most likely to depart from the ideal gas behavior? Why?
2. Out of all the "8" gases [Argon, Hydrogen, Nitrogen, Oxygen, Air, Helium, Methane, Carbon Dioxide], which one is the most likely to behave closest to that of an ideal gas? Why?
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch4/deviation5.html
Scroll down the page to the graph that is shown. PV/RT graphed vs P should be a straight line at 1.000. Looks from the graph as if CO2 deviates most and N2 deviates the least. Can you think why this might be so?
hahah
1. The gas most likely to depart from ideal gas behavior among the mentioned options is carbon dioxide (CO2). This is mainly because carbon dioxide is a relatively polar molecule due to its bent molecular shape and the presence of carbon-oxygen double bonds. Polar molecules such as CO2 tend to exhibit stronger intermolecular forces, leading to deviations from ideal gas behavior. Additionally, at high pressures and low temperatures, CO2 can undergo phase transitions to form solid or liquid states, which further deviates from the assumptions of an ideal gas.
2. Among the given options, helium (He) is the gas that behaves closest to that of an ideal gas. It possesses several characteristics that contribute to its ideal gas behavior. Firstly, helium is a monoatomic gas, meaning that it consists of single atoms without any bonds. As monatomic gases have minimal intermolecular forces, they closely obey the ideal gas law. Moreover, helium atoms are small and have low molecular mass, leading to weaker intermolecular interactions, which contribute to its ideal gas behavior. Additionally, helium is chemically inert and does not undergo chemical reactions, further supporting its ideal gas-like behavior.
To determine which gas is most likely to depart from ideal gas behavior and which gas behaves closest to an ideal gas, we need to consider certain factors. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
1. The gas most likely to depart from ideal gas behavior:
To determine this, we need to consider the conditions under which a gas deviates from ideal behavior. Typically, gases tend to deviate from ideal behavior at high pressures and low temperatures. Additionally, if the gas molecules have strong intermolecular forces or significant molecular size, they are more likely to deviate from ideality.
From the given list of gases, the gas that is most likely to depart from ideal gas behavior is Carbon Dioxide (CO2). Carbon Dioxide molecules have a larger size compared to the other gases in the list, and they have relatively stronger intermolecular forces (due to their polarity). These factors contribute to deviations from ideal gas behavior at certain conditions.
2. The gas most likely to behave closest to an ideal gas:
To determine this, we need to consider gases that exhibit properties similar to those of an ideal gas. An ideal gas behaves in a way that the gas particles occupy negligible volume, there are no intermolecular forces between them, and collisions are completely elastic.
From the given list of gases, the gas that exhibits properties closest to an ideal gas is Helium (He). Helium is an inert gas with low molecular weight and relatively weak intermolecular forces. Its small size and low interaction potential make it behave closer to the ideal gas behavior under typical conditions.
It's important to note that while Helium behaves closest to an ideal gas, no real gas perfectly follows the ideal gas behavior. All gases, to some extent, deviate from ideality under certain conditions due to various factors like molecular interactions and volume.