For an ideal gas of one mole,what is the value of \(P(\frac{dV}{dT})_{P}\) is equal to when the pressure of the gas is maintained constant?

For an ideal gas, the value of ((dU)/(dV))_(T) is:

For adiabatic process of an ideal gas the value of (dP)/P is equals to

One mole of an ideal gas requires 207 J heat to raise the temperature by 10K When heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by 5K, then the heat required is

If an ideal gas is heated at constant pressure :

One mole of an ideal gas has an interal energy given by U=U_(0)+2PV , where P is the pressure and V the volume of the gas. U_(0) is a constant. This gas undergoes the quasi - static cyclic process ABCD as shown in the U-V diagram. The molar heat capacity of the gas at constant pressure is

One mole of an ideal gas has an interal energy given by U=U_(0)+2PV , where P is the pressure and V the volume of the gas. U_(0) is a constant. This gas undergoes the quasi - static cyclic process ABCD as shown in the U-V diagram. The work done by the ideal gas in the process AB is

For an ideal gas, number of moles per litre in terms of its pressure P, gas constant R and temperature T is

An ideal gas at pressure P and temperature T is enclosed in a vessel of volume V. Some gas leaks through a hole from the vessel and the pressure of the enclosed gas falls to P'. Assume that the temperature of the gas remains constant during the leakage. What is the number of moles of the gas that have leaked ?

For an ideal gas number of moles per litre in terms of its pressure P gas contant R and temperature T is .