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° 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...
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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
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