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(B) Real gases behave ideally under conditions of low pressure and high volume,as the intermolecular forces become negligible and the volume of gas mo

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At very low temperature,real gases show ideal behaviour

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(B) Real gases behave ideally under conditions of low pressure and high volume,as the intermolecular forces become negligible and the volume of gas molecules becomes insignificant compared to the total volume of the container.At $Boyle's$ temperature,the effects of intermolecular forces and molecular volume cancel out,leading to ideal behavior.However,at very low temperatures,the kinetic energy of gas molecules decreases,making intermolecular forces significant,which causes real gases to deviate from ideal behavior.Therefore,the statement that real gases show ideal behavior at very low temperature is incorrect.

Among the following,the incorrect statement is:

Similar Questions

Identify the correct variation of pressure $(p)$ and volume $(V)$ of a real gas $(A)$ and an ideal gas $(B)$ at constant temperature. ($y = p$; $x = V$)

At low pressures,van der Waals' equation is written as $(P + \frac{a}{V^2})V = RT$. The compressibility factor $Z$ will be

Gas deviates from ideal gas nature because molecules

For which of the following is the van der Waals equation valid?

Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.

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