In: Chemistry
The enthalpy of reaction for HCN(aq) + OH-(aq) -> CN-(aq) + H2O(l) is -12.1 kJ/mol. Assuming that the correct enthalpy of reaction of the experiment is -54.0 kJ/mol, calculate the enthalpy change for the ionization of HCN:
HCN(aq) -> H+(aq) + CN-(aq)
Be sure to report your answer to the correct number of significant figures.
ΔH = ____ kJ/mol
consider the given reaction
HCN + OH- ---> CN- + H20 (l)
enthalpy of this reaction is -12.1 kJ/mol
but
the correct enthalpy of reaction of the experiment is -54 kJ/mol
So
the missing energy is used for the ionization of HCN
HCN --> H+ + CN-
so
enthalpy change for ionization of HCN = enthalpy of the reaction - correct enthalpy of the reaction
so
enthalpy change for ionization of HCN = -12.1 - (-54)
enthalpy change for ionization of HCN = 41.9
so
the enthalpy change for ionization of HCN is 41.9 kJ/mol
so
the answer is dH = 41.9 kJ/mol