Real gases deviated from ideal behaviour due to the following two faulty assumptions of kinetic theory of gases : (i) Actual volume occupied by the gas molecule is negligible as compared to the total volume of the gases (ii) Forces of attraction and repulsion among gas molecules are negligible To explain the extent of deviation of the real gas from ideal behaviour in terms of compressibility or compression factor (z), which is the function of pressure and temperature for real gases z = (P_(0)V_(0))/(nRT) For ideal gases z = 1. for real gases either z gt 1 " or " z gt 1. When z gt 1, then it is less compressible because force of repulsion dominates over force of attraction. When z lt 1, force of attraction dominates over the repulsion and it is more compressible. Graph in between z and P is shown below on increasing the temperature, z increases and approaches to unity. Graph between z and p at different temperature are as under Answer the following questions on the basis of above write up : What is correct increasing order of liquefibility of the gases shown in the above graph ?