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- Aug 19, 2013
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So the question is about a gas that has 10 L at ATP and is pressurized to 500 atm . The options are
A) V = 0.020
or B) V > 0.02 L b/c of volumes of gas molecules
or C ) V > 0.02 b/c of repulsions between individual gas molecules..
it's B not C. Why isn't it C? If you pressurize it, ideal volume is 0.02 L but it's not b/c the closer the gas molecules are to each other, the more they will repel each other. The actual answer explanation for B is
"The ideal gas law makes the assumption that molecules have no volume. This assumption is adequate when the gas is at 1 atm but when pressure is increased to 500 atm the volume of the gas molecules is no longer neglible"
This makes no sense to me. I feel like the repulsions are far more important.!
Please help. Thanks!
A) V = 0.020
or B) V > 0.02 L b/c of volumes of gas molecules
or C ) V > 0.02 b/c of repulsions between individual gas molecules..
it's B not C. Why isn't it C? If you pressurize it, ideal volume is 0.02 L but it's not b/c the closer the gas molecules are to each other, the more they will repel each other. The actual answer explanation for B is
"The ideal gas law makes the assumption that molecules have no volume. This assumption is adequate when the gas is at 1 atm but when pressure is increased to 500 atm the volume of the gas molecules is no longer neglible"
This makes no sense to me. I feel like the repulsions are far more important.!
Please help. Thanks!