Entropy Change in Thermodynamics

What is the value of ∆S0 for a reaction with ∆G = 0 at 9900°C?

A. Positive

B. Negative

C. Zero

D. Indeterminate

Answer:

The value of ∆S° for a reaction that has a Gibbs free energy change (∆G) of 0 at 9900°C is indeterminate without additional information on ∆H° or other relevant data.

The student's question pertains to the value of the entropy change (∆S°) for a reaction that has a Gibbs free energy change (∆G) equal to 0 at 9900°C. In thermodynamics, the relationship between these variables is given by the equation ∆G° = ∆H° - T∆S°. If ∆G is zero, this implies that ∆H° = T∆S°, which allows us to solve for ∆S°.

Since temperature (T) is a positive number, and at equilibrium ∆H° is likely to be a positive or negative number, ∆S° would thus also be positive or negative accordingly. However, without the value of ∆H° or additional information, the exact sign of ∆S° cannot be determined from the information given. Therefore, the correct answer would be Indeterminate (D).