for a chemical reaction aa b at a constant pressure 1 bar and a constant temperature 300 k the c

For a chemical reaction aa b at a constant pressure 1 bar...

For a chemical reaction: Aà B, at a constant pressure (1 bar) and a constant temperature (300 K), the change of enthalpy of the reaction . The change of entropy of the reaction is . Determine the change of the Gibbs free energy of the reaction: ________. Question 13 options: -3897 J/mol It cannot be determined. 0 J/mol -900 J/mol

Consider the following chemical reaction: 2H2(g) + O2(g) → 2H2O(g). Calculate the Gibbs free energy change for the reaction at 100.0°C when 4.00 mol of gaseous H2O is formed at 100.0°C and 1.00 atm from O2(g) and H2(g) at the same temperature and each at a partial pressure of 1.00 atm. It is given that the entropy change, ΔS, for the chemical reaction (see above) at 100.0°C is -93.18 J/K. The molar enthalpy of formation (ΔH°f) for H2O(g) at 25°C and 1 atm is -241.818 kJ/mol. For O2(g) and H2(g), the molar enthalpy of formation is 0.0 kJ/mol. The molar entropy of formation (ΔS°f) at 25°C and 1 atm for H2O(g), O2(g), and H2(g) are 188.72 J/K/mol, 205.04 J/K/mol, and 130.57 J/K/mol, respectively. The molar heat capacities at constant pressure (Cm,P) at 25°C for H2O(g), O2(g), and H2(g) are 33.6 J/K/mol, 29.4 J/K/mol, and 28.8 J/K/mol, respectively. Consider the heat capacities constant throughout the temperature range of the problem.

Shaiju T.

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