What is the ∆g for the following reaction between o3 and o2? 3o2(g) 2o3(g) given: o3: ∆h = 285.4 kj ∆s = -137.14 j/k)109.5 kj208.3 kj300.2 kj326.3 kj

We’ll be using the equation:
dG = dH - TdS (replace ‘d’ with triangle)

I’m going to assume 0 degrees Celsius.
At 0 C (273 K):

dG = dH - TdS
dG = (285,400 J) - (273 K)(-137.14 J/K)
dG = 285,400 J + 37,439.2 J
dG = 322,839.2 J or 322.84 kJ

The dG of this reaction is +322.84 kJ. This reaction is not considered spontaneous.

This answer, in this instance, would be D. If the temperature used in the question is not 0 degrees C, replace the temperature that I used for calculation with the Kelvin temperature given in the problem (K = C + 273), and simplify to find the answer.

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