Question

Use the standard reaction enthalpies given below to determine ?H° rxn for the following reaction: 8 SO3(g) ? 8 S(s) + 12 O2(g) ?H°rxn = ? Given: SO2(g) ? S(s) + O2(g) ?H°rxn = +296.8 kJ 2 SO2(g) + O2(g) ? 2 SO3(g) ?H°rxn = -197.8 kJ 3166 kJ -494.6 kJ -3166 kJ -791.4 kJ -692.4 kJ

          Use the standard reaction enthalpies given below to determine ?H° rxn for the following reaction:

8 SO3(g) ? 8 S(s) + 12 O2(g) ?H°rxn = ?
Given:
SO2(g) ? S(s) + O2(g) ?H°rxn = +296.8 kJ
2 SO2(g) + O2(g) ? 2 SO3(g) ?H°rxn = -197.8 kJ

3166 kJ
-494.6 kJ
-3166 kJ
-791.4 kJ
-692.4 kJ

Use the standard reaction enthalpies given below to determine ?H° rxn for the following reaction:

8 SO3(g) ? 8 S(s) + 12 O2(g) ?H°rxn = ?
Given:
SO2(g) ? S(s) + O2(g) ?H°rxn = +296.8 kJ
2 SO2(g) + O2(g) ? 2 SO3(g) ?H°rxn = -197.8 kJ

3166 kJ
-494.6 kJ
-3166 kJ
-791.4 kJ
-692.4 kJ

Added by Erica H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

07/29/2023

Step 1

We can break down the reaction into a series of steps, for which we have the enthalpy changes: Show more…

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Use the standard reaction enthalpies given below to determine ΔH° rxn for the following reaction: SO3(g) + 8 S(s) + 12 O2(g) → 5 SO2(g) Given: ΔH°f(SO2(g)) = -494.6 kJ/mol ΔH°f(S(s)) = 0 kJ/mol ΔH°f(O2(g)) = 0 kJ/mol ΔH°f(SO3(g)) = -791.4 kJ/mol ΔH°f(SO3(s)) = -692.4 kJ/mol ΔH°rxn = ΣΔH°f(products) - ΣΔH°f(reactants) ΔH°rxn = [5ΔH°f(SO2(g))] - [ΔH°f(SO3(g)) + 8ΔH°f(S(s)) + 12ΔH°f(O2(g))]