For a certain chemical reaction, ΔH∘=−39.0kJ and ΔS∘=−84.0J/K Calculate ΔG∘ for the reaction at 298 K. Is the reaction spontaneous at 298 K under standard conditions?
For a certain chemical reaction, ΔH∘=−39.0kJ and ΔS∘=−84.0J/K Calculate ΔG∘ for the reaction at 298 K....
For the values give for ΔH and ΔS, calculate ΔG foreach for each of the following reactions at 298 K. If the reactionis not spontaneous under standard conditions at 298 K, at whattemperature (if any) would the reaction become spontaneous? a) 2PbS(s)+3O2(g) ---> 2PbO(s)+2SO2(g) ΔH= -844kj ; ΔS = -165 J/K b)2POCl3(g)--->2PCl3(g)+O2(g) ΔH= 572kJ ; ΔS= 179 J/K
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?
Calculate ΔG° for a reaction that has a ΔS° of 142.6 J/K and a ΔH° of 95.7 kJ occurring at standard conditions.
Use the data in Appendix B in the textbook to calculate ΔH∘ and ΔS∘ for each of the following reactions. From the values of ΔH∘ and ΔS∘, calculate ΔG∘ at 25 ∘C and predict whether each reaction is spontaneous under standard-state conditions. Part A 2SO2(g)+O2(g)→2SO3(g) Express your answer using four significant figures. ΔH∘ = kJ Part B Express your answer using four significant figures. ΔS∘ = J/K Part C Express your answer using four significant figures. ΔG∘ = kJ Part...
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?
If ΔH = -70.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
If ΔH = -70.0 kJ and ΔS = -0.300 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
If ΔH = -80.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature Express your answer numerically in kelvins.
For the reaction: C(s) + H2O(g) CO(g) + H2(g), ΔH° = 131 kJ and ΔS° = 128 J/K at 298 K. At temperatures greater than ______ K, this reaction is spontaneous under standard conditions. a. 1.02 K b. 273 K c. 1023 K d. 753 K
Part C If ΔH = -80.0 kJ and ΔS = -0.200 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.