By increasing the temperature of a gas by 6 ^oC, its pressure increases by 0.4% at constant volume. Then the initial temperature of the gas is:

(1) 1000 K

(2) 2000 K

(3) 1500 K

(4) 750 K

Boyle's law is obeyed by:

(1) Real gas of constant mass and temperature.

(2) Ideal gas of constant mass and temperature.

(3) Both ideal and real gases at constant temperature and variable mass.

(4) Both ideal and real gases of constant mass and variable temperature.

For an ideal gas, the fractional change in its volume per degree rise in temperature at constant pressure is equal to [T is the absolute temperature of the gas]:

(1) T⁰

(2) T

(3) T^-1

(4) T²

The rise in the temperature of a given mass of an ideal gas at constant pressure and at temperature 27 ^oC to double its volume is:

(1) 327^oC

(2) 54^oC

(3) 300^oC

(4) 600^oC

A container has N molecules at absolute temperature T. If the number of molecules is doubled but kinetic energy in the box remains the same as before, the absolute temperature of the gas is:

(1) T

(2) $\frac{T}{2}$

(3) 3T

(4) 4T

During an experiment, an ideal gas is found to obey an additional law VP² = constant. The gas is initially at temperature T and volume V. When it expands to volume 2V, the resulting temperature is:

(1) $\frac{T}{2}$

(2) 2T

(3) $\sqrt{2}T$

(4) $\frac{T}{\sqrt{2}}$

When the pressure remaining constant, at what temperature, will the r.m.s. speed of gas molecules increases by 10% of the r.m.s. the speed at NTP?

(1) 81.5 K

(2) 81.5 ^oC

(3) 815.3 K

(4) -81.5 ^oC

Select the appropriate property of an ideal gas.

(1) Its molecules are infinitesimally small.

(2) There are no forces of interaction between its molecules.

(3) It strictly obeys the ideal gas laws.

(4) All of these

A real gas behaves as an ideal gas at:

(1) Very low pressure and high temperature.

(2) High pressure and low temperature.

(3) High pressure and high temperature.

(4) Low pressure and low temperature.

A gas at a pressure P₀ is contained in a vessel. If the masses of all the molecules are halved and their velocities doubled, then the resulting pressure P will be:

(1) 4P₀

(2) 2P₀

(3) P₀

(4) $\frac{{\mathrm{P}}_0}{2}$