Chapter 5 Principles of Chemical Reactivity: Energy and Chemical Reactions - Study Questions - Page 217e: 73

$-0.63\ kJ$

Enthalpies of formation (kJ/mol): $SnCl_4(l):-511.3, SnO_2(s): -577.63, H_2O(l): -285.83, HCl(aq): -167.59$ Reaction: $SnCl_4(l)+2\ H_2O(l)\rightarrow SnO_2(s)+4\ HCl(aq)$ Enthalpy change: $4\times-167.59+ -577.63-2\times -285.83- -511.3=-165.03\ kJ/mol$ For 1.00 g: $(1.00\ g\div 260.51\ g/mol)\times -165.03\ kJ/mol=-0.63\ kJ$