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# Calculate delta G; temperature; pressure

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Kp is 1.0x10-3 atm-1/2 at 2000K and delta S at standard temperature and pressure = 87.864 J/K mole (delta Cp = 0) for the reaction
CO2(g) yielding CO(g) + 1/2 O2(g) (this reaction is reversible)

(a) Calculate delta G at 2000K,
(b) Calculate delta G at standard temperature and pressure at 298K, and
(c) Calculate the degree of dissociation of CO2 if the equilibrium mixture is brought to 2000K and 2 atm total pressure (assume enthalpy and entropy are temperature independent)

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This solution is provided in 643 words. It demonstrates how to solve the problem and uses an attached .doc file as a tutorial for how free energy and temperature change are related to entropy.

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Thank you.

Ok, the missing piece in my mind is the thought that the enthalpy and the entropy change for the reaction is essentially constant over the temperature range given The clue that delta Cp is zero makes this necessary. However, the literature actually cites that delta Cp for a temperature change is not zero for this reaction.

The attachment discusses the major change in the free energy is a result of the product of the change in temperature with a constant change in entropy resultant from the reaction and not the temperature change.

(a) Calculate delta G at 2000K,
(b) Calculate delta G at standard temperature and pressure at 298K, and
(c) Calculate the degree of dissociation of CO2 if the equilibrium mixture is brought to 2000K and 2 atm ...

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