**Problem Statement:**What is the ΔS° if the ΔH° is -199 kJ and ΔG° is -197.78 kJ?**Options:**- a) 25 J/K- b) -25 J/K- c) +0.25 J/K- d) 4.1 J/K- e) -4.1 J/K**Explanation:**The question involves determining the change in entropy (ΔS°) for a reaction given the changes in enthalpy (ΔH°) and Gibbs free energy (ΔG°). It seems to be related to thermodynamics, where the formula used is:\[ \Delta G° = \Delta H° - T\Delta S° \]Rearrange the formula to solve for ΔS°:\[ \Delta S° = \frac{\Delta H° - \Delta G°}{T} \]Given:- ΔH° = -199 kJ- ΔG° = -197.78 kJTo solve the problem, substitute values and calculate ΔS°. Note: Ensure units are consistent for accurate calculation. The temperature (T) may be needed or assumed if not provided.

Given data : deltaG° = -197.78 KJ deltaH° = -199 KJ T = 25°C = 298 K (standard temperature)…

Answered: What is the AS° if the AH° is -199 kJ…

What is the AS° if the AH° is -199 kJ and AG ° is -197.78 kJ? a) 25 J/K Ob) -25 J/K c) +0.25 J/K d) 4.1 J/K O e) -4.1 J/K

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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