Answer: The value of enthalpy of the given reaction is 44.000 kJ/mol , that is energy is supplied to water to change into water vapors
Explanation:
\(H_2O(l)\rightarrow H_2O(g),\Delta H_{rxn}=?\)
Enthalpy of formation of water in liquid state,\(\Delta H_{f,H_2O(l)}=-285.820 kJ/mol\)
Enthalpy of formation of water in gaseous state,\(\Delta H_{f,H_2O(g)}=-241.820 kJ/mol\)
\(\Delta H_{rxn}=\sum \Delta H_f \text{of products}-\sum \Delta H_f \text{of reactants}\)
\(\Delta H_{rxn}=(-241.820 kJ/mol)-(-285.820 kJ/mol)=44.000 kJ/mol\)
The value of enthalpy of the given reaction is 44.000 kJ/mol, that is energy is supplied to water to change into water vapors.
