When 100 mL of 1.0 M HCl was mixed with 100 mL of 0.1 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7^(@)C was measured for the beaker and its contents. Because the enthypy of neutralization of a strong acid with a strong base is a constant (-57.0" kJ mol"^(-1)), this experiment could used to measure the calorimeter constant. In a second experiment 100 mL of 2.0 M acetic acid (K_(a)=2.0xx10^(-5)) was mixed with 100 mL of 1.0 M NaOH (under identical conditions of Expt. 1) where a temperature rise of 5.6^(@)C 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 from the Expt. 2 is

When 100 mL of 1.0 M HCl was mixed with 100 mL of 0.1 M NaOH in an ins

1.	When 100 mL of 1.0 M HCl was mixed with 100 mL of 0.1 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7^(@)C was measured for the beaker and its contents. Because the enthypy of neutralization of a strong acid with a strong base is a constant (-57.0" kJ mol"^(-1)), this experiment could used to measure the calorimeter constant. In a second experiment 100 mL of 2.0 M acetic acid (K_(a)=2.0xx10^(-5)) was mixed with 100 mL of 1.0 M NaOH (under identical conditions of Expt. 1) where a temperature rise of 5.6^(@)C 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 from the Expt. 2 is
Answer» `1.0` `10.0` `24.5` `51.4` ANSWER :A