Select incorrect statement(s):a)At very low pressure real gases show minimum deviation from ideal behaviour.b)Real gas show maximum deviation at high pressure and low temperaturec)At Boyle temperature real gas behave as ideal gas in high pressure regiond)The compressibility factor for an ideal gas is zeroCorrect answer is option 'D'. Can you explain this answer?

Question

Answer

Corrected Answer:

The correct statement is option D, which states that real gases show maximum deviation at high pressure and low temperature.

Explanation:

Real gases do not strictly adhere to the ideal gas laws at all conditions, especially at high pressures and low temperatures. The deviations from ideal behavior are due to the presence of intermolecular forces and the finite size of gas molecules.

Deviation from Ideal Behavior:

- At very low pressure: Real gases show minimum deviation from ideal behavior. This is because the molecules are far apart from each other and the intermolecular forces are negligible. The volume occupied by the gas molecules becomes insignificant compared to the total volume, and the gas behaves like an ideal gas.

- Compressibility factor for an ideal gas is zero: The compressibility factor, Z, is defined as the ratio of the actual volume of a gas to the volume predicted by the ideal gas law. For an ideal gas, Z is always equal to 1, not zero. This is because the ideal gas law assumes that gas molecules have no volume and do not interact with each other.

- At Boyle temperature: Real gases behave as ideal gases in the high-pressure region. The Boyle temperature is defined as the temperature at which the compressibility factor is minimum. At this temperature, the intermolecular forces are weakened, and the gas molecules occupy a smaller volume compared to their actual size. As a result, the gas behaves more like an ideal gas in the high-pressure region.

- Maximum deviation at high pressure and low temperature: Real gases show maximum deviation from ideal behavior at high pressures and low temperatures. At high pressures, the gas molecules are closer together and experience stronger intermolecular forces. These forces cause the gas to occupy a larger volume compared to the predictions of the ideal gas law. At low temperatures, the kinetic energy of the gas molecules decreases, and they move more slowly, increasing the effect of intermolecular forces. These factors contribute to the maximum deviation from ideal behavior at high pressures and low temperatures.

Overall, the behavior of real gases deviates from ideal behavior under certain conditions, particularly at high pressures and low temperatures, due to intermolecular forces and molecular size.

Answer

Incorrect statement is D. The compressibility factor for an ideal gas is zero. This statement is incorrect. The compressibility factor (Z) is defined as Z = PV/nRT. For an ideal gas, by definition, Z is equal to 1 because PV = nRT according to the ideal gas law.

Answer

Option( B )and option ( D ) both are incorrect

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