We’re being asked to **determine the heat (q) released or enthalpy change** by the reaction of **0.95 g S**

The given reaction is:

2 S (s) + 3 O_{2}(g) → 2 SO_{3}(g); ΔH˚_{rxn} = –790.0 kJ/mol

From the balanced equation, we can see that the given **ΔH˚ _{rxn} (–790.0 kJ)** corresponds to

Recall that at constant pressure, ** heat is equivalent to enthalpy**.

$\overline{){\mathbf{q}}{\mathbf{\left(}}{\mathbf{heat}}{\mathbf{\right)}}{\mathbf{}}{\mathbf{=}}{\mathbf{\u2206}}{\mathbf{H}}\left(\mathbf{enthalpy}\right)}$

The value of ΔH° for the reaction below is -790 kJ. The * enthalpy change* accompanying the reaction of 0.95 g of S is __________ kJ.

**2 S (s) + 3 O_{2} (g) → 2 SO_{3} (g)**

A. +23

B. -23

C. -12

D. +12

E. -790

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