Study the following thermochemical data: S + - ; δ H = -298.2 kJ; + 1/2 - ; δ H = -98.2 kJ; + - ; δ H = -130.2 kJ; + 1/2 - ; δ H = -287.3 kJ. The enthalpy of formation of at 298 K will be

Question

Study the following thermochemical data: S + $O_2$ -> $SO_2$; δ H = -298.2 kJ; $SO_2$ + 1/2 $O_2$ -> $SO_3$; δ H = -98.2 kJ; $SO_3$ + $H_2O$ -> $H_2SO_4$; δ H = -130.2 kJ; $H_2$ + 1/2 $O_2$ -> $H_2O$; δ H = -287.3 kJ. The enthalpy of formation of $H_2SO_4$ at 298 K will be

Prashant Kotian · Accepted Answer

Correct answer: D. We want the formation reaction of : (g) + S(s) + 2(g) -> (l). Adding the four given reactions together gives exactly this target equation. Thus, delta_f H° = -298.2 - 98.2 - 130.2 - 287.3 = -813.9 kJ/mol.

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