All the oxides of nitrogen have positive values of ΔG°_f at 298 K, but only one common oxide of nitrogen has a positive ΔS°_f. Identify that oxide of nitrogen without reference to thermodynamic data and explain.

Dinitrogen tetroxide decomposes to nitrogen dioxide: N₂O₄(g) → 2 NO₂(g) ΔH°_rxn = 55.3 kJ At 298 K, a reaction vessel initially contains 0.100 atm of N₂O₄. When equilibrium is reached, 58% of the N₂O₄ has decomposed to NO₂. What percentage of N₂O₄ decomposes at 388 K? Assume that the initial pressure of N₂O₄ is the same (0.100 atm).

Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine triphosphate (ATP). The ATP acts as an energy source for a variety of reactions that the living organism must carry out to survive. ATP provides energy through its hydrolysis, which can be symbolized as follows: ATP(aq) + H₂O(l) → ADP(aq) + P_i(aq) ΔG°_rxn = -30.5 kJ where ADP represents adenosine diphosphate and P_i represents an inorganic phosphate group (such as HPO₄^2-). b. The free energy obtained from the oxidation (reaction with oxygen) of glucose (C₆H₁₂O₆) to form carbon dioxide and water can be used to re-form ATP by driving the given reaction in reverse. Calculate the standard free energy change for the oxidation of glucose and estimate the maximum number of moles of ATP that can be formed by the oxidation of one mole of glucose.

These reactions are important in catalytic converters in automobiles. Calculate ΔG° for each at 298 K. Predict the effect of increasing temperature on the magnitude of ΔG°.

a. 2 CO(g) + 2 NO(g) → N₂(g) + 2 CO₂(g)

b. 5 H₂(g) + 2 NO(g) → 2 NH₃(g) + 2 H₂O(g)

c. 2 H₂(g) + 2 NO(g) → N₂(g) + 2 H₂O(g)

d. 2 NH₃(g) + 2 O₂(g) → N₂O(g) + 3 H₂O(g)

The values of ΔG°_f for the hydrogen halides become less negative with increasing atomic number. The ΔG°_f of HI is slightly positive. However, the trend in ΔS°_f is to become more positive with increasing atomic number. Explain.