At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behaviour. Their equation of state is given as p = 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?
Ne
Xe
Ar
Kr
Consider the following table:
Gas | a/(kPa dm6mol-1) | b/(dm3mol-1) |
A | 642.32 | 0.05196 |
B | 155.21 | 0.04136 |
C | 431.91 | 0.05196 |
D | 155.21 | 0.4382 |
And b are vander walls contants . The correct statement a Bout the gases is :
Gas A will occupy than gas D Compressible than gas D Gas C will Occupy more volume than
gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than
Gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than
Gas A: gas B will be lesser Compressble than gas D
Points I, II and III in the following plot respectively correspond to (Vmp: most probale velocity)
Vmp of N2 (300K); Vmp of O2(400K); Vmp of H2 (300K)
Vmp of N2 (300K); Vmp of H2(300K); Vmp of O2 (400K)
Vmp of H2 (300K); Vmp of N2(300K); Vmp of O2 (400K)
Vmp of O2 (400K); Vmp of N2(400K); Vmp of H2 (300K)
A.
Vmp of N2 (300K); Vmp of O2(400K); Vmp of H2 (300K)