Given below are observations on molar specific heats at room temperature of some common gases.
`{:("Gas","Molar specific heat "(C_(v))),(,("cal mol"^(1)K^(-1))),("Hydrogen",4.87),("Nitrogen",4.97),("Oxygen",5.02),("Nitric oxide",4.99),("Carbon monoxide",5.01),("Chlorine",6.17):}`
The measured molar specific heats of these gases are markedly different from those for monatomic gases. Typically, molar specific heat of a monatomie gas is` 2.52` cal/mol K. Explain this difference. What can you infer from the somewhat larger than the rest) value for chlorine ?

Explanation

The gases are diatomic, and have other degrees of freedom fic, have other modes of motion) possible besides the translational degrees of freedom. To raise the temperature of the gas by a certain amount, heat is to be supplied to increase the average energy of all the modes Consequently, molar specific heat of diatomic gases is more than that of monatomie gases. It can be shown that if only rotational modes of motion are considered, the molar specific heat of diatomic gases is nearly (5/2) R which agrees with the observations for all the gases listed in the table, except chlorine. The higher value of molar specific heat of chlorine indicates that besides rotational modes, vibrational modes are also present in chlorine at room temperature.