Use the data in the image above to decide at what temperatures does this real ga

Question

Use the data in the image above to decide at what temperatures does this real gas tend to exhibit ideal gas behavior? High or low? Explain. Use the data in the image above to decide at what pressures does real gas tend to exhibit ideal gas behavior? High or low? Explain. Which of the following statement if most correct: Gases tend to be ideal at high pressures and high temperatures Gases tend to be ideal at low pressures and low temperatures. Gases tend to be ideal at low pressures and high temperatures. Gases tend to be ideal at high pressures and low temperatures. In general, Z tends to be larger than 1 at very high pressures (greater than 350 bar for methane). Which van der Waals' factor seems to be responsible for this behavior-- a or b? Explain. In general, Z tends to be smaller then I at moderately high pressures (around 150 bar for methane). Which van der Waals' factor seems to be responsible for this behavior-- a or b? Explain.

Explanation / Answer

1) At high temperatures real gases tend to nearly idealy as the gas molecules will be moving faster ,thereby developing weak molecular forces of attractions.From graph, at high temperatures the Z vs P graph reduces its slope,until it becomes zero (as for ideal gases) at very high temperatures.

2)At low pressures, real gases tend to behave ideally as the gas molecules collisions is low and hence reduced attractions between molecules

3) c.Gases tend to be ideal at high pressures and low temperatures

4)5)At high pressure ,the factor b becomes significant as the space left for particles to move is reduced due to increased density of molecules that increases the factor b or actual volume of gas molecules

5)Z=compressibility factor =PV/nRT ,as for ideal gas PV=nRT ,so Z=1

For real gases, Z >1 at high pressures.

The vander waal factor a is the measure of average attraction between particles which exists at high pressure due to optimum collision between gas molecules.

Change of pressure at moderate pressures =(P+an^2/V^2)

So that the ideal gas equation changes to (P+an^2/V^2)(V-nb)=nRT [where b=excluded volume of gas molecules which becomes at high pressures]

As pressure is increased so Z>1

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