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The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) → NaCN(aq) + H2O(l). Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH. If the temperature of the calorimeter increases by 2.79 °C, what is the enthalpy of this neutralization reaction (in kJ/mol)? Assume the density of the solution is 1.00g/mL and that the specific heat is 4.184 J/g °C {