Question

Calculate the enthalpy change (in kJ/mol) for the ionization of sulfuric acid (H2SO4) given the following information: H2SO4 (l) → H+ (aq) + HSO4- (aq)ΔH1 = +1009 kJ/molHSO4- (aq) → H+ (aq) + SO4^2- (aq)ΔH2 = +513 kJ/mol.

Answer 1

To calculate the enthalpy change for the ionization of sulfuric acid, we need to add the enthalpy changes for the two steps involved in the process:1. H2SO4  l   H+  aq  + HSO4-  aq  with H1 = +1009 kJ/mol2. HSO4-  aq   H+  aq  + SO4^2-  aq  with H2 = +513 kJ/molThe overall reaction is:H2SO4  l   2H+  aq  + SO4^2-  aq The enthalpy change for the overall reaction is the sum of the enthalpy changes for the two steps:H_total = H1 + H2H_total =  +1009 kJ/mol  +  +513 kJ/mol H_total = +1522 kJ/molSo, the enthalpy change for the ionization of sulfuric acid is +1522 kJ/mol.