Chemistry - Thermochemistry Question with Solution | TestHub

$HCl+NaOH⟶NaCl+H_{2}O$

1 mole 1 mol 1 mol $\Delta H=-13.7$

When this heat is used to increase the temperature of 2 L solution, the temperature was $x$℃. Now, if we add 500 mL each of 1 M $H_{2}S{O}_4$ and 1 M $Ba(OH{)}_2$:

$H^{+}+O{H}^{-}⟶H_{2}O$

1 mol 1 mol 1 mol

(From $H_{2}S{O}_4$) (from $Ba(OH{)}_2$) $\Delta H=-13.7$

This heat is used to increase the temperature of 1 L solution; hence, the temperature should be double, $y=2x$.