States of Matter

The temperature at which oxygen molecules have the same root mean square speed as helium atoms have at 300 K is : (Atomic masses : He = 4 u, O = 16 u)

The initial volume of a gas cylinder is 750.0 mL. If the pressure of gas inside the cylinder changes from 840.0 mm Hg to 360.0 mm Hg, the final volume the gas will be :

Sulphur dioxide and oxygen were allowed to diffuse through a porous partition. 20 dm$^3$ of $\ce{SO2}$ diffuses through the porous partition in 60 seconds. The volume of $\ce{O2}$ in dm$^3$ which diffuses under the similar condition in 30 seconds will be (atomic mass of sulphur = 32 u) :

The succeeding operations that enable this transformation of states are

For one mole of a van der Waals gas when $b=0$ and $T=300$ K, the $PV$ vs. $1/V$ plot is shown below. The value of the van der Waals constant $a$ (atm.liter² mol⁻²) is

According to kinetic theory of gases

The term that corrects for the attractive forces present in a real gas in the van der Waals equation is

At 400 K, the root mean square (rms) speed of a gas X (molecular weight = 40) is equal to the most probable speed of gas Y at 60 K. The molecular weight of the gas Y is

A gas described by van der Waals equation

Match gases under specified conditions listed in Column I with their properties/laws in Column II. Indicate your answer by darkening the appropriate bubbles of the 4 × 4 matrix given in the ORS.