Answer:- delta H for the given reaction is -12.6 kJ/mol.
Solution:- delta H of the reaction = sum of standard enthalpy of formation of products - sum of standard enthalpy of formation of reactants
Standard enthalpy of formation values could be found in thermodynamic data table given in book.
The values for methanol, hydrofluoric acid, methylfluoride and water are -238.6 kJ/mol, -268.6 kJ/mol, -234kJ/mol and -285.8 kJ/mol respectively.
Please note, the phases taken for methanol, hydrofluoric acid, methylfluoride and water are liquid, gas, gas and liquid respectively.
Let's plug in the values in the formula.
delta H for the reaction = [(-234) +(-285.8)] - [(-238.6) + (-268.6)]
delta H for the reaction = -519.8 + 507.2
delta H for the reaction = -12.6 kJ/mol
