If for hydrogen `s_p-s_v=a` and oxygen `s_p-s_v=b`, where `s_p` and `s_v` refer to specific heats at constant pressure and at constant volume then

If for hydrogen C_p-C_v = m and for nitrogen C_p -C_v= n , where C_p and C_v refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between m and n is : (Molecular weight of hydrogen = 2 molecular weight or nitrogen = 14 )

The ratio [C_(p)//C_(v)] of the specific heats at a constant pressure and at a constant volume of any perfect gas

If for hydrogen C_(P) - C_(V) = m and for nitrogen C_(P) - C_(V) = n , where C_(P) and C_(V) refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between m and n is (molecular weight of hydrogen = 2 and molecular weight or nitrogen = 14)

If for hydrogen C_(P) - C_(V) = m and for nitrogen C_(P) - C_(V) = n , where C_(P) and C_(V) refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between m and n is (molecular weight of hydrogen = 2 and molecular weight or nitrogen = 14)

If for hydrogen C_(P) - C_(V) = m and for nitrogen C_(P) - C_(V) = n , where C_(P) and C_(V) refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between m and n is (molecular weight of hydrogen = 2 and molecular weight or nitrogen = 14)

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.

Show that for an ideal gas C_p - C_v = R where C_p and C_v are the heat capacity at constant pressure and constant volume respectively.