For a reaction for which ∆H = -142 kJ/mol and ∆S = -178 J/mol･K, which of the following statements is true? A) The reaction is spontaneous above 798 K. B) The reaction is spontaneous below 798 K. C) The reaction will never reach equilibrium. D) The reaction will never be spontaneous.

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Q: At what temperature will a reaction become spontaneous, if its AS is +100.3 J/mol and AH° is +48.90…

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Q: Consider the reaction 2Hg (l) + O2 (g) → 2HgO (s), for which ∆H°= -181.7 kJ/mol and ∆S°= -216.5…

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Q: At what temperature/temperature range does this reaction become spontaneous? Explain your reason.…

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Q: Calculate the DeltaG° rxn using the following information at 25°C. And determine wether the reaction…

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Q: Above what temperature does the following reaction become nonspontaneous?               2 H2S(g) +…

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Q: The heat of vaporization of methanol, CH3OH, is 35.20 kJ/mol. Its boiling point is 64.6°C. What is…

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Q: Calculate the free energy change for this reaction at 25 °C. Determine if the reaction is…

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Q: Find the temperatures at which reactions with the following ΔH and ΔS values would become…

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Q: The value of AHtransition of C(graphite)-C(diamond) is 1.9 kJ/mol at 25 °C. Entropy of graphite is…

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Q: One of the following processes is spontaneous at 298 K Which one? 1. H2O(l)-H2O(g, 1 atm) 2.…

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Q: estimate the temperature that one would have to heat 1 L of water to, starting at 0 °C, reversibly,…

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