From attempting to find ΔG I’ve used the equation of ΔG=ΔH-TΔS. I found the change in temp and changed the units of ΔS to kJ. The answer that I keep getting is -270.77. Which is not an answer listed and I’m not sure where I’m going wrong. Please help me find my error 1 pointConsider the following equation:S(s, rhombic ) + O2( g) → SO2( g)At 298 K, AH° for this reaction is -269.9 kJ/mol, and AS° is +11.6 J/K.What is the value of AG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide?-300.4+300.4-4,597+4,597-274.2

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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From attempting to find ΔG I’ve used the equation of ΔG=ΔH-TΔS. I found the change in temp and changed the units of ΔS to kJ. The answer that I keep getting is -270.77. Which is not an answer listed and I’m not sure where I’m going wrong. Please help me find my error

1 point
Consider the following equation:
S(s, rhombic ) + O2( g) → SO2( g)
At 298 K, AH° for this reaction is -269.9 kJ/mol, and AS° is +11.6 J/K.
What is the value of AG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide?
-300.4
+300.4
-4,597
+4,597
-274.2

Expert Solution

Step 1

We know the thermodynamic equation.,

∆G° = ∆H° - T∆S°

where,

∆H° = -269.9 KJ/mol

∆S° = +11.6 J/mol.K = +0.0116 KJ/mol.K

(1 J = 0.001 KJ then 11.6 J = 11.6 X 0.001 = 0.0116 KJ)

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