If `gamma` be the ratio of specific heats at cosntant pressure & constant volume, then show that the degree of freedom Is n = `2/(gamma-1)`

Show that the specific heat of a gas at constant pressure is greater than that at constant volume.

Define specific heat of a gas at constant volume and that at constant pressure.

The ratio between the specific heats of an ideal gas is gamma . Show that the number of degrees of freedom of the gas molecules is n=2/(gamma-1) .

The ratio between the specific heats of an ideal gas is y. show that the number of freedom of the gas molecules is n=2/(y-1)

Using first law of thermodynamics derive the relation between specific heat at constant pressure and constant volume.

Why are the specific heats of gases at constant pressure and at constant volume different? Determine the relation between these two specific heats of an ideal gas.

Show that for an ideal gas the difference between the molar heat capacities at constant pressure and at constant volume is equal to the universal gas constant (R).

What do you understand by the molar specific heat of a gas at constant volume and constant pressure?

From the relation C_p-C_v=R show that the ratio of two specific heats (gamma) of an ideal gas is given by gamma=1+2/f where f is the degrees of freedom of the molecule.

From the relation C_p - C_v= R show that the ratio of two specific heats (gamma) of an ideal' gas is given by gamma = 1+ 2/ f , where f is the degrees of freedom of a molecule.