I am revising and am a bit stumped by this thermodynamics questions-Question
The molar constant pressure heat capacities (Cp) of molecular and atomic iodine in the temperature range 900-1100K are approximately 9R/2 and 5R/2 respectively.
Explain why this should be so and write down an expression that relates the enthalpy of dissociation of I2
at a temperature T (in the range 900K-1100K) to the enthalpy of dissociation at 1000K.Thoughts
I thought that at higher temperature there were more degrees of freedom (not less) and that for a linear molecule the maximum degrees of freedom was 5R/2 due to translations+rotations. Is Cp= Cv+nR relevant?
For the second part is it just Kirchoff's law?
Any help really appreciated