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Posted by on Sunday, October 5, 2008 at 5:15pm.

Why do gases behave in a less ideal manner when in LOW TEMP. AND HIGH PRESSURE?

  • Chemistry - , Sunday, October 5, 2008 at 5:19pm

    Dont real gas molecules occupy volume, and have attractive forces? Do real gases become liquids? Why? Ideal gases cant do this.

  • Chemistry - , Sunday, October 5, 2008 at 5:22pm

    I don't know what you just said, but i know that when an ideal gas is at a lower pressure, the molecules do not collide with the container as frequently, and that at a high temperature the molecules do collide frequently. What does this mean, does it even help me?

  • Chemistry - , Sunday, October 5, 2008 at 5:28pm

    No. Reread what I asked. I gave you the answer. If you have no idea what I am writing of, you quickly need to reread your text on the failure of the assumptions of the ideal gas vs real gases.

  • Chemistry - , Sunday, October 5, 2008 at 5:37pm

    Ok, i understand that for real gases you have to account for volume of particles, and that they have attractive forces that lower the pressure, that make the ideal gas law invalid, but what does that have to do with low temp and high pressure?

  • Chemistry - , Sunday, October 5, 2008 at 5:50pm

    Is it because at high pressure, molecules have volume, and at low temperature gases move slowly and act like a liqud so they have attractive forces that decrease pressure?

  • Chemistry - , Sunday, October 5, 2008 at 5:36pm

    Ok, i understand that for real gases you have to account for volume of particles, and that they have attractive forces that lower the pressure, that make the ideal gas law invalid, but what does that have to do with low temp and high pressure?

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