COMPRESSIBILITY FACTOR

Determine which of the following statements are true at very high pressure for a real gas: (a) Compressibility factor is greater than 1. (b) Compressibility factor varies linearly with pressure. (c) Molar volume occupied by gas is more as compared to ideal gas at similar pressure and temperature. (d) Gas is less compressible as compare to ideal gas. (e) Compressibility factor is given by Z=1+(Pb)/(RT) .

Match the compression factor under different condition (in List-I) with its value (in List-II)

At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behavior. Their equation of state is given as P = (RT)/(V-b) at T. Here, b is the van der Waals constant. Which gas will exhibit steepest increase in the plot of Z (compression factor) vs P?

Boyle's temperature or Boyle point is the temperature at which a real gas starts behaving like an ideal gas over a particular range of pressure. A graph is plotted between compressibility factor Z and pressure P. What is the deviation of real gas from ideal behaviour in terms of compressibility factor , Z ?

Two equal-volume flasks A and B containing equal masses of H_(2) and CH_(4) are at 100 K and 200 K , respectively. Assuming ideal behaviour, which of the following statements about the compressibility factor ( Z ) is true?

Boyle's temperature or Boyle point is the temperature at which a real gas starts behaving like an ideal gas over a particular range of pressure. A graph is plotted between compressibility factor Z and pressure P. What is the variation of Z with pressure ?

The density of vapour of a substance (X) at 1 atm pressure and 500 K is 0.8 kg//m^(3) . The vapour effuse through a small hole at a rate of 4//5 times slower than oxygen under the same condition. What is the compressibility factor (z) of the vapour ?

The critical pressure P_(C) and critical temperature T_(C) for a gas obeying van der Waal's equation are 80 atm at 87^(@) C. molar mass of the gas is 130 g/mole. The compressibility factor for the above gas will be smaller than unity under the following condition:

Homogeneous mixing and compressibility both result from the fact that the molecules are far apart in gases. Mixing occurs because individual gaseous molecules have little interaction with their neighbours, assuming that no reaction taken place, the chemical identities is possible in gases because only about 0.1% of the volume of a typical gas is taken up by the molecules themselves under normal circumstances, the remaining 99.9% is empty space Compressibility factor of a gas is given by

For critical constant factor, compression factor Z is