Question

When a chemist mixed 3.35 g of LiOH and 165 mL of 0.65 M HCl in a constant-pressure calorimeter, the final temperature of the mixture was 25.8°C. Both the HCl and LiOH had the same initial temperature, 21.2°C. The equation for this neutralization reaction is:

LiOH(s) + HCl(aq) → LiCl(aq) + H₂O(l).

Given that the density of each solution is 1.00 g/mL and the specific heat of the final solution is 4.1801 J/g·K, calculate the enthalpy change for this reaction in kJ/mol LiOH. Assume no heat is lost to the surroundings.

_____ kJ/mol LiOH