Thermodynamics ...

Pressure versus temperature graphs of an ideal gas are as shown in figure. Choose the wrong statement:-

If the temperature difference $$T_1 - T_2$$ is $$120^oC$$. the temperature difference between points A & B is 

When volume of system is increased two times and temperature is decreased half of its initial temperature, then pressure becomes  

A rigid diatomic ideal gas undergoes an adiabatic process at room temperature,. The relation between temperature and volume of this process is $$TV^x$$ = constant, then $$x$$ is :

An ideal gas of adiabatic exponent $$\gamma $$ is supplied heat at a constant pressure. Then ratio dQ : dQ : dU is equal to :

An ideal gas is enclosed in a cylinder at pressure of 2 atm and temperature, 300 K. The mean time between two successive collisions is $$6\times 10^{ -8 }$$ s. If the pressure is doubled and temperature is increased to 500 K, the mean time between two successive collisions will be close to :

A vessel contains $$N$$ molecules of a gas at temperature $$T$$. Now the number of molecules is doubled, keeping the total energy in the vessel constant. The temperature of the gas is.

At ordinary temperature, the molecule of an ideal gas has only translational and rotational kinetic energies. At high temperatures, they may also have vibrational energy. As a result of this at higher temperatures ( = molar heat capacity at constant volume)

If the number of molecules of $$\mathrm { H } _ { 2 }$$ are double than that of $$\mathrm { O } _ { 2}, $$ then ratio of mean kinetic energy per molecule of hydrogen to that of oxygen at 300$$\mathrm { K }$$ is 

The equation of process in terms of volume and temperature is: