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
Above what temperature does the following reaction become nonspontaneous? 2H2S(g) + 3O2(g) →2SO2(g) + 2H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K
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.
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
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)
Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below: 2H2S(g) + 4O2(g) → 2SO3(g) + 2H2O(l) Report your answer to three significant figures in scientific notation. Equations: ΔH°rxn (kJ) 2S(s) + 3O2(g) → 2SO3(g) -790.4 S(s) + O2(g) → SO2(g) -296.9 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(l) -1125.1
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