An ideal gas has molar constant-volume specific heat equal to 2.5 times the universal gas constant, R = 8.314 J/(mol K). If its temperature rises by 100 K, find its change in molar specific enthalpy in J/mol.
For an ideal gas, $c_p=c_v+R=(2.5+1)R=3.5R$. Enthalpy depends only on temperature, so $\Delta h=c_p\Delta T=3.5(8.314)(100)=2909.9$ J/mol. Using $c_v$ would give internal-energy change rather than enthalpy change.
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