The basis to settle this question is the Gibbs Free Energy relation between the adjust in enthalpy , ΔH, and the adjust in entropy ΔS, through the relation

ΔG = ΔH - TΔS ( T is temperature )

For a provided reaction ΔG should be negative for the reactivity to be positive.

So to deal with our question we have to identify the authorize for the change in complimentary energy studying whether the enthalpy is positive or positive, and also doing the exact same with the term TΔS.

You are watching: Classify the possible combinations of signs for a reaction

A. ΔH positive, ΔS negative ⇒ ΔG : always positive non spontaneous.

B.

ΔH positive, ΔS positive ⇒ If TΔS > ΔH, ΔG is negative spontaneous

If TΔS ΔH, ΔG is positive nonspontaneous

Then,

1. Spontaneous as created at all temperatures: C

2. Spontaneous in reverse at all temperatures: A

3. Spontaneous as created above a specific temperature : B

4. Spontaneous as created below a certain temperature : D


Sfinish
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In the attached image, you will certainly find the solution for this exercise.

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