Problem: 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 O2 (g) → 2 SO3 (g)A. +23B. -23C. -12D. +12E. -790

FREE Expert Solution

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 O2(g)  2 SO3(g); ΔH˚rxn = –790.0 kJ/mol


From the balanced equation, we can see that the given ΔH˚rxn (–790.0 kJ) corresponds to 2 moles of S


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

q(heat) =Henthalpy


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Problem Details

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 O2 (g) → 2 SO3 (g)

A. +23
B. -23
C. -12
D. +12
E. -790

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