Determine ΔG◦rxn using the following information.
2H2S(g)+3O2(g) ---> 2H2O(l)+2SO2(g) ΔH= +1.12kJ ;ΔS=
-390.7J/K
ΔG = ΔH - T x ΔS
Here, considering reaction happen at T = 273 K
ΔH= +1.12kJ = + 1120.0 J
ΔS = - 390.7 J/K
ΔG = (1120 J) - (273 x - 390.7) = 1120 - (- 106661.1) = 1120 +106661.1 = 107781.1 J = + 107.78 kJ
Important to Notice: Temperature considered as =0 oC = 273 K
If you change the Value of T, Delta G will changes.
Determine ΔG◦rxn using the following information. 2H2S(g)+3O2(g) ---> 2H2O(l)+2SO2(g) ΔH= +1.12kJ ;ΔS= -390.7J/K
Determine delta G(not) rxn using the following information. Assume standard cognitions. 2H2S(g) +3O2(g) --> 2H2O(l)+2SO2(g) Delta H (not): 1.12 kJ Delta S(not): -390.7 J/K
Calculate ΔS∘rxn for the following balanced chemical equation: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance and state S∘[J/(K⋅mol)] H2O(g) 188.8 O2(g) 205 H2S(g) 205.7 SO2(g) 248.1
Calculate ΔG° (kJ/mole) at 298 K for the reaction below:2H2S(g) + 3O2(g) ⇋2H2O(g) + 2SO2(g)K=6.32×1010Enter a number to 2 decimal places.
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
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 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)
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
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C.? 2CH4(g)→C2H6(g)+H2(g) Part B: Calculate ΔS∘rxn at 25 ∘C 2NH3(g)→N2H4(g)+H2(g) Part B: Calculate ΔS∘rxn at 25 ∘C.
For the reaction: 2H2S(g) + 3O2(g)2H2O(g) + 2SO2(g) deltaH = -1.04×103 kJ and S° = -153 J/K The equilibrium constant, K, would be greater than 1 at temperatures (above, below) _____ Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.