An endothermie process that decreases in entropy is always nonspontaneous. Why can't we determine a temperature at which it shifts to being spontancous? An endothermic process has a positive AH. A increase in entropy has a positive AS. If we plug this into the equation, it will give us a negative value for temperature, which is not possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero, An endothermic process has a positive AH. A decrease in entropy has a negative AS. If we plug this into the equation, it will give us a negative value for temperature, which is not possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero. s An endothermic process has a positive AS. A decrease in entropy has a negative AH. If we plug this into the equation, it will give us a negative value for temperature, which is possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero, d. None of the above

An endothermie process that decreases in entropy is always nonspontaneous. Why can't we determine a temperature at which it shifts to being spontancous? An endothermic process has a positive AH. A increase in entropy has a positive AS. If we plug this into the equation, it will give us a negative value for temperature, which is not possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero, An endothermic process has a positive AH. A decrease in entropy has a negative AS. If we plug this into the equation, it will give us a negative value for temperature, which is not possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero. s An endothermic process has a positive AS. A decrease in entropy has a negative AH. If we plug this into the equation, it will give us a negative value for temperature, which is possible because the temperature is in Kelvin, and the lowest value that it can acquire is zero, d. None of the above

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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According to the second law of thermodynamics for any spontaneous process, the entropy of the universe (increases, decreases, or remains constant)
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8 As you dissolve salt in water, what change would you expect to occur? A B C D The entropy of the system will increase. The kinetic energy of the water molecules decreases. The salt consumes energy as it transfers entropy The water molecules become more closely packed as the temperature increases
Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)
1
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