**Problem Statement:**Consider a chemical reaction that has a ΔH° = 30.0 kJ/mol and a ΔS° = 100.0 J/(mol•K). At what temperature does this reaction become spontaneous?**Options:**- ○ 2.00 x 10² K- ○ 3.00 x 10³ K- ○ 1.30 x 10² K- ○ 7.00 x 10¹ K- ○ 3.00 x 10² K**Explanation:**To determine the temperature at which the reaction becomes spontaneous, you will use the Gibbs free energy equation:\[ \Delta G = \Delta H - T \Delta S \]A reaction is spontaneous when \(\Delta G < 0\).Given:- \(\Delta H° = 30.0 \text{ kJ/mol} = 30000 \text{ J/mol}\)- \(\Delta S° = 100.0 \text{ J/(mol•K)}\)Set the equation to zero and solve for \(T\):\[ 0 = 30000 - T \times 100 \]\[ T = \frac{30000}{100} = 300 \text{ K} \]Thus, the temperature at which the reaction becomes spontaneous is 300 K.

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Answered: Consider a chemical reaction that has a…

Chemistry

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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

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

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