Enthalpy changes

The equation for the reaction of barium hydroxide with hydrochloric acid is shown below:

\text{Ba(OH)}_2(\text{aq}) + 2\text{HCl}(\text{aq}) \rightarrow \text{BaCl}_2(\text{aq}) + 2\text{H}_2\text{O}(\text{l})

A volume of 80.0 cm³ of 0.250 mol dm^-3 $Ba(OH)2\text{Ba(OH)}_2$ is reacted with excess $HCl\text{HCl}$ . The heat energy released is 2.256 kJ.

What is the standard enthalpy change of neutralisation, in $mol−1\text{kJ mol}^{-1}$ ?

$- 112.8$

$- 56.4$

$+ 56.4$

$- 225.6$

The equation for the reaction of barium hydroxide with hydrochloric acid is shown below:

\text{Ba(OH)}_2(\text{aq}) + 2\text{HCl}(\text{aq}) \rightarrow \text{BaCl}_2(\text{aq}) + 2\text{H}_2\text{O}(\text{l})

A volume of 80.0 cm³ of 0.250 mol dm^-3 $Ba(OH)2\text{Ba(OH)}_2$ is reacted with excess $HCl\text{HCl}$ . The heat energy released is 2.256 kJ.

What is the standard enthalpy change of neutralisation, in $mol−1\text{kJ mol}^{-1}$ ?

$- 112.8$

$- 56.4$

$+ 56.4$

$- 225.6$

Enthalpy changes Questions