At what temperature and pressure the behaviour of a real gas closest to that of an ideal gas?
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A real gas approaches the behavior of an ideal gas more closely at conditions like higher temperatures and low pressures.
It is important that the molecules of the real gas are far apart so that they don’t attract each other very strongly and they don’t take up a large fraction of the volume, in order to behave like an ideal gas.
An ideal gas a hypothetical gas whose molecules occupy negligible space and have no interactions, and which consequently obeys the gas laws exactly. Real gases are non-hypothetical gases whose molecules occupy space and have interactions; consequently, they adhere to gas laws.
It is important that the molecules of the real gas are far apart so that they don’t attract each other very strongly and they don’t take up a large fraction of the volume, in order to behave like an ideal gas.
An ideal gas a hypothetical gas whose molecules occupy negligible space and have no interactions, and which consequently obeys the gas laws exactly. Real gases are non-hypothetical gases whose molecules occupy space and have interactions; consequently, they adhere to gas laws.
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Well, there are different pressure and temperature for every gas to behave like an ideal gas . Basically the conditions to be followed in this regard is that the intermolecular forces become zero and also the size of the gas must be close to zero that;s mean volume of the must be zero. As the temperature of the gas increased and their pressure in decreased it become more towards like a ideal gas So at very low pressure and high temperature a gas can act like a ideal gas . This can be represented in the form of PV/nRT must be equal to 1.
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