Prove that `C_(p) - C_(v) = R` , where `C_(p) and C_(v)` are the molar specific heats at constant pressure and constant volume respectively and R is the universal gas constant.

Prove C_(p) - C_(v) = R

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?

An ideal gas undergoes a quasi-static, reversible process in which its molar heat capacity C remains constant. If during this process the relation of pressure p and volume V is given by pV^(n) = constant, then n is given by (Here C_(p) and C_(v) are molar specific heat at constant pressure and constant volume, respectively)

The dimension of R (universal gas constant) is-

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.

C_(v) and C_(p) denote the molar specific heat capacities of a gas at constant volume and constant volume and constant pressure, respectively. Then,

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

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