3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, 4G, is -228.57 kJ.mot', for a standard state of 1 atm. The reaction is: 2 H;0 (g) O (g) + 2H, (g) (a) Calculate 4 G° (kJ.mol) for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K at 5 atm.

Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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Chapter17: Chemcial Thermodynamics
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3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, 4G, is -228.57 kJ.mot', for a
standard state of 1 atm. The reaction is: 2 H30 (g) - O (g) + 2H, (g)
(a) Calculate 4 G° (kJ.mol) for the above reaction.
(b) Calculate the value of the equilibrium constant, K, for the above reaction.
(c) Calculate the value of K at 5 atm.
Transcribed Image Text:3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, 4G, is -228.57 kJ.mot', for a standard state of 1 atm. The reaction is: 2 H30 (g) - O (g) + 2H, (g) (a) Calculate 4 G° (kJ.mol) for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K at 5 atm.
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