Substance ΔH (kJ/mole) ΔS (J/mole∙K) A2B(g) 25.0 200. AB(g) 50.0 175. A2 (g) 0 100. A) Calculate the entropy, ΔS, for this reaction at 298 K. B) Calculate the enthalpy, ΔH, for this reaction at 298 K. C) Calculate the Gibbs free energy for this reaction at 298 K. D) Is this reaction thermodynamically favorable? E) Without performing any calculations, will the value for K be greater than 1 or less than
I know this is a long question...can you dock me 2 questions so I don't have to re-write it?
Given the following reaction and table of
2 A2B(g) ⇌ 2 AB(g) + A2(g)
| Substance | ΔH (kJ/mole) | ΔS (J/mole∙K) |
| A2B(g) | 25.0 | 200. |
| AB(g) | 50.0 | 175. |
| A2 (g) | 0 | 100. |
A) Calculate the entropy, ΔS, for this reaction at 298 K.
B) Calculate the enthalpy, ΔH, for this reaction at 298 K.
C) Calculate the Gibbs free energy for this reaction at 298 K.
D) Is this reaction thermodynamically favorable?
E) Without performing any calculations, will the value for K be greater than 1 or less than 1? Explain.
F) Calculate the value for K.
G) When the reaction reaches equilibrium, will the reactants or the products be favored?
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I got 50 J/mol K for a. using your math... is that correct?
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