For a reaction, ΔH = – 249 kJ and ΔS = – 278 J/K.
What is the maximum temperature at which the reaction is spontaneous?
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For the reaction ΔH°=+61.14 kJ and ΔS° = +132 J/K at 25°C. At what For the reaction ΔH°=+61.14 kJ and ΔS° = +132 J/K at 25°C. At what minimum temperature will the reaction be spontaneous?minimum temperature will the reaction be spontaneous? Select one: a. 479 K b. 500 K c. 463 K d. 571 K e. 2904 K
For a particular reaction, ΔH° is -28.4 kJ and ΔS is -87.9 J/K. Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?
Part A: ΔH∘rxn= 121 kJ ; ΔS∘rxn=− 246 J/K ; T= 291 K Express your answer as an integer. Part B: ΔH∘rxn=− 121 kJ ; ΔS∘rxn= 246 J/K ; T= 291 K Express your answer as an integer. Part C: ΔH∘rxn=− 121 kJ ; ΔS∘rxn=− 246 J/K ; T= 291 K Express your answer as an integer. Part D: ΔH∘rxn=− 121 kJ ; ΔS∘rxn=− 246 J/K ; T= 600 K Express your answer as an integer. Part E: Predict whether...
A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign and magnitude of ΔH and ΔS, will the reaction be spontaneous at all temperatures, nonspontaneous at all temperatures? Briefly explain your reasoning. b. Calculate the standard free energy change for the reaction at 298 K. c. Is the reaction spontaneous or nonspontaneous at 298 K?
For a given reaction, ΔH = +20.8 kJ and ΔS = +27.6 J/K. The reaction is spontaneous __________ A) At T < 754 K B) At T > 133 K C) At all temperatures D) At T > 754 K E) At T < 133 K
For a particular reaction, ΔH∘=−28.4 kJΔH∘=−28.4 kJ and ΔS∘=−87.9 J/K.ΔS∘=−87.9 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous?
For a particular reaction, ΔH = -32 kJ and ΔS =-98 J/K. Assume that ΔH and ΔS do not vary withtemperature. A) At what temperature will the reaction have ΔG= 0? B) If T is increased from that in part A, will the reaction bespontaneous or nonspontaneous?
Consider a reaction for which ΔH = 6.03 kJ/mol; ΔS = 22.1 J/K-mol. Which of the following statements is true? a. The reaction becomes spontaneous at high temperatures above 273 K b. The reaction becomes spontaneous at low temperatures below 273 K c. The reaction is spontaneous at all temperatures d. The reaction is never spontaneous
If ΔH = -70.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?