#comprehension type

In the following reactions

Compound X is

Compound Y is

When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of \(5.7^oC\) was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (\(- 57 kJ mol^{-1}\)), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (\(K_a = 2.0 \times 10^{-5}\)) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of \(5.6^oC\) was measured. (Consider heat capacity of all solutions as \(4.2 J g^{-1} K^{-1}\) and density of all solutions as \(1.0 g mL^{-1}\))

Enthalpy of dissociation (\(in \ kJ mol^{-1}\)) of acetic acid obtained from Expt. 2 is A) 1.0 B) 10.0 C) 24.5 D) 51.4