Homework Answers
At extremely high pressures, the molar volumes of a real gas deviates from that of an ideal gas. This can be explained on the
basis of the following postulate of the Kinetic Molecular Theory.
"The gas particles are much smaller than the distance between particles. Most of the volume of a gas is therefore empty space. "
At extremely high pressures, the above postulate is not true. The distance between particles becomes comparable to the volume
of the gas particles. Hence, most of the volume of a gas is not empty space. So deviations are observed from ideal behaviour.
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At very high pressures (M 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because Multiple Choice such high pressures cannot be accurately measured. ces real gases will condense to form liquids at 1000 atm pressure. gas phase colisions prevent molecules from colliding with the walls of the container. of attractive intermolecular forces between gas molecules KPrev 6 of 10 Next> Multiple ChOice SUch high pressures cannot...
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2. The gas laws are defined for ideal gases. Real gases do not always follow the gas laws exactly Under what conditions would you predict that real gases least approximate ideal gas behavior Explain why real gases behave least like ideal at the conditions you stated. 3. Define molar mass including the units in which it is expressed. on produced a 0.311 g sample of gas which occupied 225 ml at 55°C exerting a pressure of 886 mm Hg. What...
Which of the following statements is true tor real gases? Choose all that apply. As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. Attractive forces between molecules cause a decrease in pressure compared to the ideal gas. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas. As molecules increase in size. deviations from ideal behavior become more apparent at relatively low pressures.
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