An ideal gas cannot be liquified because                                          

1. its critical temperature is always above 0$°$C

2. its molecules are relatively smaller in size

3. it solidifies before becoming a liquid

4. forces operating between its molecules are negligible

The correct value of the gas constant 'R' is close to 

1. 0.082 L atm K

2. 0.082 L atm K^-1 mol^-1

3. 0.082 L atm^-1 K mol^-1

4. 0.082 L^-1 atm^-1 K mol

While He is allowed to expand through a small jet under adiabatic condition heating effect is observed. This is due to the fact that:

1. helium is an inert gas

2. helium is a noble gas

3. helium is an ideal gas

4. the inversion temperature of helium is very low

The condition that favour a pure sample of an ideal gas to have pressure of 1 atm and a concentration of

1 mol L^-1  is -

(R=0.082 L atm mol^-1K^-1)                                     

1. At STP

2. When V = 22.4 L

3. When T = 12 K

4. Impossible under any conditions

If an open container is heated from 300 K to 400 K, then the % of gas that remains in the container is-

1. 25%

2. 50%

3. 75%

4. 100%

1.6 g O₂ gas and 0.1 g H₂ gas are placed in a 1.12 L flask at 0 ^oC. The total pressure of the gas mixture will be-

1. 2 atm

2. 3 atm

3. 4 atm

4. 1 atm

An open flask containing air is heated from 300 K to 500 K. The percentage of air that will escape into the atmosphere if pressure is kept constant is-

1. 80

2. 40

3. 60

4. 20

A collapsed polythene bag of 30 litre capacity is partially blown up by the addition of 10 litre of N₂ at 0.965 atm at 298 K. Subsequently,  enough O₂  is pumped into bag so that at 298 K and external pressure of 0.990 atm, the bag contains full 30 litre. The final pressure of O₂ in the following experiment is-

60 mL of a mixture of equal volume of Cl₂ and an oxide of chlorine was heated and then cooled back to the original temperature. The resulting gas mixture was found to have volume of 75 ml. On treatment with caustic soda solution, the volume contracted to 15 ml. Assume that all the measurements are made at same T and P. Deduce the simplest formula for oxide of Cl₂. The oxide of Cl₂ on heating decomposes quantitatively to O₂ and Cl₂.

An underwater bubble with radius of  5 cm at the bottom of tank , where the temperature is 5^oC and pressure is 3 atm rises to the surface, where temperature is 25 ^oC and pressure is 1 atm. What will be the radius of bubble when it reaches to the surface?