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1.The van der Waals equation (or van der Waals equation of state; named after Johannes Diderik van der Waals) is an equation of state that generalizes the ideal gas law based on plausible reasons that real gases do not act ideally.
2.The constants are the characteristic of the individual gas. When gas is ideal or that it behaves ideally then both the constant will be zero. Generally, a constant help in the correction of the intermolecular forces while the b constant helps in making adjustments for the volume occupied by the gas particles.
3.The two condition at which the gases deviate from ideal behaviour are low temperature and high pressure. At high pressure and at low temperature the volume is less, so the volume occupied by the individual molecule can not be neglected compare to the total volume.
4.Real gases behaves like ideal gases at higher temperature and lower pressure. Low pressure decreases the effect of finite size of real particles by increasing volume around each particle. High temperature provides enough kinetic energy to particle to overcome real attractions existing between particles.
5.The compressibility factor (Z) is a useful thermodynamic property for modifying the ideal gas law to account for behavior of real gases. It is a measure of how much the thermodynamic properties of a real gas deviate from those expected of an ideal gas.
6.The compressibility factor (Z) is a useful thermodynamic property for modifying the ideal gas law to account for behavior of real gases. It is a measure of how much the thermodynamic properties of a real gas deviate from those expected of an ideal gas. It may be thought of as the ratio of the actual volume of a real gas to the volume predicted by the ideal gas at the same temperature and pressure as the actual volume is ( refer the picture)
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