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For the reaction H2(g) + S(s) --> H2S(g), ΔH° = -20.2 kJ/mol and ΔS° = +43.1 J/K·mol. Which of these statements is true?  Select one: a. ΔG° becomes less favorable as temperature increases. b. The reaction is at equilibrium at 25°C under standard conditions. c. The reaction is only spontaneous at low temperatures. d. The reaction is spontaneous only at high temperatures. e. The reaction is spontaneous at all temperatures.

For the reaction H2(g) + S(s) --> H2S(g), ΔH° = -20.2 kJ/mol and ΔS° = +43.1 J/K·mol. Which of these statements is true?  Select one: a. ΔG° becomes less favorable as temperature increases. b. The reaction is at equilibrium at 25°C under standard conditions. c. The reaction is only spontaneous at low temperatures. d. The reaction is spontaneous only at high temperatures. e. The reaction is spontaneous at all temperatures.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter21: Chemistry Of The Nonmetals
Section: Chapter Questions
Problem 53QAP: Consider the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (a) Calculate ?H° for this reaction. Is it...
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For the reaction H2(g) + S(s) --> H2S(g), ΔH° = -20.2 kJ/mol and ΔS° = +43.1 J/K·mol.

Which of these statements is true? 


Select one:
a. ΔG° becomes less favorable as temperature increases.
b. The reaction is at equilibrium at 25°C under standard conditions.
c. The reaction is only spontaneous at low temperatures.
d. The reaction is spontaneous only at high temperatures.
e. The reaction is spontaneous at all temperatures.
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