The heat capacity of one mole an ideal is found to be CV = 3R (1 + aRT)/2 where a is a constant. The equation obeyed by this gas during a reversible adiabatic expansion is -

The heat capacity at constant volume of an ideal gas consisting of monatomic molecules is 3//2 R ( where R is the gas constant ) . The heat capacity at constant pressure is :

For certain process the molar heat capacity of an ideal gas is found to be (C_v+R/2) , where C_v is the molar heat capacity of the same gas at constant volume. For the given process, it can be concluded that

During an adiabatic reversible expansion of an ideal gas

During an adiabatic reversibly expansion of an ideal gas

During an adiabatic reversibly expansion of an ideal gas

One mole of a monoatomic ideal gas is expanded by a process described by PV^(3) = C where C is a constant. The heat capacity of the gas during the process is given by (R is the gas constant)

The molar heat capacity C for an ideal gas going through a given process is given by C=a/T , where 'a' is a constant. If gamma=C_p/C_v , the work done by one mole of gas during heating from T_0 to eta T_0 through the given process will be

The molar heat capacity C for an ideal gas going through a given process is given by C=a/T , where 'a' is a constant. If gamma=C_p/C_v , the work done by one mole of gas during heating from T_0 to eta T_0 through the given process will be