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All of the following statements are correct, except
- a)reduced pressure is a dimensionless quantity.
- b)all gases have compressibility factor of nearly unity at high temperature and pressures.
- c)the van der Waal's gas three roots of identical values at the critical point.
- d)in case of real gases, the deviation from the ideal conditions is maximum when each of the reduced pressure and reduced temperature has unit value.
Correct answer is option 'B'. Can you explain this answer?
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All of the following statements are correct, excepta)reduced pressure ...
Explanation:
Option B states that all gases have a compressibility factor of nearly unity at high temperature and pressures. This statement is incorrect because the compressibility factor, also known as the Z-factor, is a measure of how much a real gas deviates from ideal gas behavior. It is defined as the ratio of the actual volume of a gas to the volume it would occupy if it behaved ideally at the same temperature and pressure.
The compressibility factor is given by the equation:
Z = PV/RT
where P is the pressure, V is the volume, R is the gas constant, and T is the temperature. For an ideal gas, the compressibility factor is always equal to 1. However, for real gases, the compressibility factor can deviate from unity due to intermolecular interactions and the finite size of gas molecules.
At high temperatures and pressures, the compressibility factor of a real gas can deviate significantly from unity. This is because the intermolecular forces become more significant, and the gas molecules are closer together, leading to deviations from ideal gas behavior. Therefore, option B is incorrect.
The other statements are correct, and we can explain them briefly as follows:
a) Reduced pressure is a dimensionless quantity:
The reduced pressure is defined as the ratio of the actual pressure to the critical pressure of a gas. It is a dimensionless quantity because it is the ratio of two pressures with the same units.
b) The van der Waals gas has three roots of identical values at the critical point:
The van der Waals equation of state is a modification of the ideal gas law that takes into account the intermolecular forces and the finite size of gas molecules. At the critical point, which is the temperature and pressure at which the gas and liquid phases coexist in equilibrium, the van der Waals equation has three roots, and these roots have identical values.
c) In the case of real gases, the deviation from ideal conditions is maximum when each of the reduced pressure and reduced temperature has a unit value:
The reduced pressure and reduced temperature are dimensionless quantities that are used to account for the effects of pressure and temperature on the behavior of real gases. When both the reduced pressure and reduced temperature have a value of unity, the deviation from ideal gas behavior is maximum.
In conclusion, all of the given statements are correct except for option B, which states that all gases have a compressibility factor of nearly unity at high temperature and pressures.
Option B states that all gases have a compressibility factor of nearly unity at high temperature and pressures. This statement is incorrect because the compressibility factor, also known as the Z-factor, is a measure of how much a real gas deviates from ideal gas behavior. It is defined as the ratio of the actual volume of a gas to the volume it would occupy if it behaved ideally at the same temperature and pressure.
The compressibility factor is given by the equation:
Z = PV/RT
where P is the pressure, V is the volume, R is the gas constant, and T is the temperature. For an ideal gas, the compressibility factor is always equal to 1. However, for real gases, the compressibility factor can deviate from unity due to intermolecular interactions and the finite size of gas molecules.
At high temperatures and pressures, the compressibility factor of a real gas can deviate significantly from unity. This is because the intermolecular forces become more significant, and the gas molecules are closer together, leading to deviations from ideal gas behavior. Therefore, option B is incorrect.
The other statements are correct, and we can explain them briefly as follows:
a) Reduced pressure is a dimensionless quantity:
The reduced pressure is defined as the ratio of the actual pressure to the critical pressure of a gas. It is a dimensionless quantity because it is the ratio of two pressures with the same units.
b) The van der Waals gas has three roots of identical values at the critical point:
The van der Waals equation of state is a modification of the ideal gas law that takes into account the intermolecular forces and the finite size of gas molecules. At the critical point, which is the temperature and pressure at which the gas and liquid phases coexist in equilibrium, the van der Waals equation has three roots, and these roots have identical values.
c) In the case of real gases, the deviation from ideal conditions is maximum when each of the reduced pressure and reduced temperature has a unit value:
The reduced pressure and reduced temperature are dimensionless quantities that are used to account for the effects of pressure and temperature on the behavior of real gases. When both the reduced pressure and reduced temperature have a value of unity, the deviation from ideal gas behavior is maximum.
In conclusion, all of the given statements are correct except for option B, which states that all gases have a compressibility factor of nearly unity at high temperature and pressures.
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All of the following statements are correct, excepta)reduced pressure is a dimensionless quantity.b)all gases have compressibility factor of nearly unity at high temperature and pressures.c)the van der Waals gas three roots of identical values at the critical point.d)in case of real gases, the deviation from the ideal conditions is maximum when each of the reduced pressure and reduced temperature has unit value.Correct answer is option 'B'. Can you explain this answer?
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