Given the thermodynamic data in the table below, calculate the standard Gibbs free energy change at 298 K (in kJ/mol) for the reaction: C;H2 (g) + H2 (g) – C;Ha (g) (R = 0.082 atm.L/K.mol = 8.314 J/K.mol) * Substance AH°i (kJ/mol) S° (J/K.mol) CH, (g) CH, (g) H2 (g) 226.7 200.8 52.30 219.4 130.58 - -112.0 O 33.2 D -141.0 ) -1.4 x 105 D -174.4

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Q: At what temperatures will a reaction be spontaneous if ΔrH° = +62.4 kJ and ΔrS° = +301 J/K?

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Q: calculate Gibbs free energy change in KJmol^-1 . The temperature for the reaction is 425k.

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Q: For the chemical system: KOH + HBr → KBĽ¢ + H,O + 45 kJ (aq) (aq) (1) which of the following is…

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