Gaseous State

For gaseous state, if most probable speed is denoted by C*, average speed by $\mathop C\limits^{\_\_}$ and mean square speed by C, then for a large number of molecules the ratios of these speeds are:

Initially, the root mean square (rms) velocity of N₂ molecules at certain temperature is $u$. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms, then the new rms velocity will be :

In Van der Waals equation of state of the gas law, the constant ‘b’ is a measure of

'a’ and `b’ are van der Waals’ constants for gases. Chlorine is more easily liquefied than ethane because

The compressibility factor for a real gas at high pressure is :

If Z is a compressibility factor, van der Waals equation at low pressure can be written as:

At very high pressures, the compressibility factor of one mole of a gas is given by :

Consider the following table : .tg {border-collapse:collapse;border-spacing:0;border-color:#9ABAD9;} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:#9ABAD9;color:#444;background-color:#EBF5FF;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:#9ABAD9;color:#fff;background-color:#409cff;} .tg .tg-s6z2{text-align:center} Gas a/(k Pa dm⁶ mol⁻¹) b/(dm³ mol⁻¹) A 642.32 0.05196 B 155.21 0.04136 C 431.91 0.05196 D 155.21 0.4382 a and b are vander Waals constants. The correct statement about the gases is :

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 $p = {{RT} \over {V - b}}$ 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?

The volume of gas A is twice than that of gas B. The compressibility factor of gas A is thrice than that of gas B at same temperature. The pressures of the gases for equal number of moles are -