Chemistry - Thermochemistry Question with Solution | TestHub

Given that

(i) Heat of solution for $A{B}_{(s)}$ is $-0.95\times 10^{X}kcal/mol$

(ii) Lattice energy for $A{B}_{(s)}$ is $700kcal/mol$. $A{B}_{(s)}⟶A^{+}(g)+B^{-}(g)$, $\Delta H=+700kcal/mol$

(iii) $A^{+}(g)⟶A^{+}(aq)$, $\Delta H=-1000kcal/mol$

$B^{-}(g)⟶B^{-}(aq)$, $\Delta H=-650kcal/mol$

then calculate the value of ’ x’.