1. The problem statement, all variables and given/known data WHat is the molar enthalpy of neutralization of NaOH (aq) when 50.0 mL of aqueous 1.00 mol/L of NaOH (aq) reacts with an excess of 1.00 mol/L H2SO4 (aq)? Initial temperature of H2SO4 - 21.3 degrees celcius Initial Temperature of NaOH - 20.6 degrees celcius Final temperature of solution - 28 degrees celcius 2. Relevant equations n(molar enthalpy) = vc(change in temperature) Where c = 4.19 J/mL x degrees celcius 3. The attempt at a solution molar enthalpy = ( vct) / (n) = ( 50 mL x 4.19 (28 - (21.3 + 20.6 / 2)) / (1.00 mol/L x 50.0 mL) = 29 KJ / mol I'm not entirely sure if this answer and its units are correct, or if averaging the two initial temperatures was correct. Any verification of my answer would be great.