A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes. The acid-base reaction is as follows: 2NaOH(aq)+ H2SO4 → Na2SO4(aq)+ 2H2O(l)

The temperature of each solution before mixing is 22.3°C. After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C. Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g•°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction.