Kinetic Theory ...

A quantity of heat 'Q' is suppplied to a monotomic ideal gas which ecpands at constant pressure. The fractionm of heat that goes into workdone by the gas is 

'n' moles of an ideal gas undergoes a process A $$\rightarrow$$B as shown in figure. The maximum temperature of the gas during the process will be :

One mole of an ideal monoatomic gas is heated at a constant pressure of one atmosphere from $${0}^{o}C$$ to $${100}^{o}C$$. Then the change in the internal energy is

A circular disc of mass $$m$$ and radius $$r$$ is rolling about its axis with a constant speed $$v$$. Its kinetic energy is 

A monoatomic ideal gas undergoes a process given by $$2dU+3dW=0$$ then the process is:

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:

What amount of heat must be supplied to 35 g of oxygen at room temperature to raise its temperature by $${ 80 }^{ \circ  }C$$ at constant volume (molecular mass of oxygen is 32 and R = 8.3 J $${ moI }^{ -1 }{ K }^{ -1 }$$)

When work done by a system was 10 J, the increase in the internal energy of the system was 30 J. The heat 'q' supplied to the system was :

The kinetic energy of molecular translation per unit volume of a gas at 2 atmosphere pressure will be nearly 

A fixed mass of gas is taken through a process $$A\rightarrow B\rightarrow C\rightarrow A$$. Here $$A\rightarrow B$$ is isobaric $$B\rightarrow C$$ is adiabatic and $$C\rightarrow A$$ is isothermal

The pressure at $$C$$ is given by $$(\gamma=1.5)$$