7) The equilibrium constant for a chemical reaction was found to depend on tempera- ture over the temperature range 400 K to 600 K according to the following equation: In K(T) = A + B T C T² where A, B, and C are the constants A = −3.53, B = −2736 K, and C = 2.2 × 105 K². Calculate the standard reaction enthalpy and the standard reaction entropy at T = 500 K.

7. The vapor pressure of benzene between 10 °C and 30 °C fits the expression 1780 K log()= 7.960- T where T is in K. Calculate (a) the enthalpy of vaporization (Avap H) and (b) the normal boiling point of benzene.

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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) ⇒ 2NH₂(g) the standard change in Gibbs free energy is AG° = −32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH₂ = 0.750 atm? AG = 737 kJ/mol

Rt is 0.616 T is 37c G=G+RT * ln(k)

Calculate the standard Gibbs reaction energy for the reaction at 298 K, 2CH3CHO(g) + O2(g) - > 2CH3 COOH(I) Given the following data, Sm\deg (CH3CHO(g )) = 250.30 J K-1 mol-1 Sm\deg (O2(g)) = 205.10 JK -1 mol-1 Sm\deg (CH3COOH(l))=159.80~K-1~mol-1\backslash Delta fHm\deg (CH3CHO(g))=-166.20~kJ~mol-1\backslash Delta fHm\deg (O2(g)) = 0.00 kJ mol-1 \Delta fHm\ deg (CH3COOH(I)) = 484.50 kJ mol-1