A reaction has ΔH∘rxn=−237 kJ and ΔS∘rxn= 218 J/K. Calculate ΔG∘rxn at 60 ∘C.
Assume there is no chang ein H and S with respect of T
T = 60°C = 60+273 = 333 K
then
G = H - TS is valid
H = -237000 J
S = 218 J/K
then
G = -237000 -333*218 = -309594 J
G = -309.59 kJ
A reaction has ΔH∘rxn=−237 kJ and ΔS∘rxn= 218 J/K. Calculate ΔG∘rxn at 60 ∘C.
Calculate ΔG° at 298.0 K for this reaction given that ΔH°rxn = –12.0 kJ and ΔS°rxn = –147 J/K
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C? N2(g)+O2(g)→2NO(g) Express your answer using three significant figures. ΔH∘rxn ΔHrxn∘ = 183 kJ SubmitPrevious Answers Correct Part H Part complete Calculate ΔS∘rxn at 25 ∘C. Express your answer to one decimal place....
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.
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...
Given the information A+B⟶2D. ΔH∘=−794.8 kJ ΔS∘=377.0 J/K C⟶D. ΔH∘=449.0 kJΔS∘=−192.0 J/K calculate ΔG∘ at 298 K for the reaction A+B⟶2C
Given the values of ΔH∘rxn, ΔS∘rxn, and T , determine ΔSuniv: A) ΔH∘rxn=− 124 kJ , ΔS∘rxn= 258 J/K , T= 298 K B) ΔH∘rxn= 124 kJ , ΔS∘rxn=− 258 J/K , T= 298 K C)ΔH∘rxn=− 124 kJ , ΔS∘rxn=− 258 J/K , T= 298 K D) H∘rxn=− 124 kJ , ΔS∘rxn=− 258 J/K , T= 554 K
Given the values of ΔH∘rxn,ΔS∘rxn, and T below, determine ΔSuniv A) ΔH∘rxn = 125 kJ , ΔS∘rxn = −257 J/K , T= 296 K . B) ΔH∘rxn= −125 kJ, ΔS∘rxn= 257 J/K, T=296 K. C) ΔH∘rxn= −125 kJ, ΔS∘rxn= -257 J/K, T=296 K. D) ΔH∘rxn= −125 kJ, ΔS∘rxn= -257 J/K, T=561 K.
2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 29 ∘C. Express your answer using four significant figures. Part A ΔG = ______ kJ Part B Is the reaction spontaneous? spontaneous OR nonspontaneous
Consider the following reaction: 2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K Calculate the free energy change for the reaction at 32 ∘C.
2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 17 ∘C. Express your answer using four significant figures. ΔG = _____kJ