For the reaction:\[ 2\text{Na}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{NaOH}(aq) + \text{H}_2(g) \]\[\Delta H^\circ = -368.6 \, \text{kJ} \quad \text{and} \quad \Delta S^\circ = -15.3 \, \text{J/K}\]The standard free energy change for the reaction of 1.87 moles of $\text{Na}(s)$ at 300 K, 1 atm would be $\_\_\_\_) \, \text{kJ}$.This reaction is $\_\_\_\_$ favored under standard conditions at 300 K.Assume that $\Delta H^\circ$ and $\Delta S^\circ$ are independent of temperature.Buttons: - Submit Answer- Retry Entire GroupNote: 9 more group attempts remaining.

Answered: Image /qna-images/answer/ef1b938e-f6dc-419b-9ff1-f20203554bcb.jpg

Use the References to access important values if needed for this question. For the reaction 2Na(s) + 2H₂O(1)→ 2NaOH(aq) + H₂(g) AH = -368.6 kJ and AS° = - 15.3 J/K The standard free energy change for the reaction of 1.87 moles of Na(s) at 300 K, 1 atm would be kJ. This reaction is standard conditions at 300 K. Assume that AH° and AS° are independent of temperature. favored under Submit Answer 9 more group attempts remaining Retry Entire Group

Use the References to access important values if needed for this question. For the reaction 2Na(s) + 2H₂O(1)→ 2NaOH(aq) + H₂(g) AH = -368.6 kJ and AS° = - 15.3 J/K The standard free energy change for the reaction of 1.87 moles of Na(s) at 300 K, 1 atm would be kJ. This reaction is standard conditions at 300 K. Assume that AH° and AS° are independent of temperature. favored under Submit Answer 9 more group attempts remaining Retry Entire Group

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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