For the water gas reaction C (s) + H2O (g) <-> CO (g) + H2 (g)At 1000 K the standard Gibbs free energy change of the reaction is - 8.314 kJ/mol. Therefore at 1000 K the equilibrium constant of the above water gas reaction is:
Correct answer: D. 2.718
- A. 1
- B. 10
- C. 1/e
- D. 2.718
Explanation
∆rGº = - 8.314 × 103∴- ∆rGº = 8.314 × 103 = RT ln Keqor 8.314 × 103 = 8.314 × 103 ln Keqor ln Keq = 1 = ln e or Keq = e = 2.718
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About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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