For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC.
Multiple Choices:
ΔS = -174 J/K
ΔS = -0.174 J/K
ΔS = -2.08J/K
ΔS = 174 J/K
ΔS = -2080 J/K
G = H - TS
-514 kJ = -566 kJ - 298*S
S = (-514000 + 560000)/(-298) = -174.5J/molK
choose dS = -174.5J/molK
For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC....
1. For the reaction 2SO2(g) + O2(g) ----->2SO3(g) ΔG° = -148.8 kJ and ΔS° = -187.9 J/K at 261 K and 1 atm. The maximum amount of work that could be done by this reaction when 1.98 moles of SO2(g) react at standard conditions at this temperature is _______ kJ. 2. For the reaction 2Na(s) + 2H2O(l) ---->2NaOH(aq) + H2(g) ΔH° = -368.6 kJ and ΔS° = -15.3 J/K The maximum amount of work that could be done when 2.25...
Calculate ΔG° at 298.0 K for this reaction given that ΔH°rxn = –12.0 kJ and ΔS°rxn = –147 J/K
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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.
Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K (Hint- What is the temperature when measuring standard heat of energy and change in entropy) Determine the equilibrium constant for the following reaction at 298 K. SO3(g) + H2O(g) → H2SO4(l) ΔG° = -90.5 kJ 7.31 × 1015 0.964 1.37 × 10-16 4.78 × 1011
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Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K (Hint- What is the temperature when measuring standard heat of energy and change in entropy)
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
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 = -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?