Van der waal equation becomes approximately PV=nRT
Hence gases behave ideally at high temperature and low pressure.
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Similar Questions
Q1
A gas behaves more closely as an ideal gas at
(a) low pressure and low temperature
(b) low pressure and high temperature
(c) high pressure and low temperature
(d) high pressure and high temperature.
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Q2
Which of the following behaves as an ideal gas under high temperature and low pressure?
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Q3
A gas is said to behave like an ideal gas when the relation PVT=constant. When do you expect a real gas to behave like an ideal gas
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Q4
Assertion: Gasses obey Boyle's law at high temperature and low pressure only.
Reason: At low pressure and high temperature, gasses would behave like ideal gases.
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Q5
Assertion :Real gases behave as ideal gases most closely at low pressure and high temperature. Reason: Intermolecular force between ideal gas molecules is assumed to be zero.