In state A, two ideal gases (represented by yellow and green spheres) initially occupy two separate bulbs. When the stopcock is opened, the two ideal gases went from state A to state B. Relate states A and B to the graph.

At constant temperature, an ideal gas undergoes expansion. Determine the signs (+, −, or 0) of ΔS, ΔH, and ΔG for this process.

Determine at which point/s labeled a through e in the graph of the total free energy of reactants and products versus the reaction progress is Q > K.

Which of the following statement is true about the reaction shown below?

N₂O₄(g) → 2 NO₂(g) ΔH° = 58.02 kJ; ΔS° = 176.6 J/K

Predict which temperature condition is needed for the reaction below be spontaneous: 

2 CO(g) + O₂(g) → 2 CO₂(g) (exothermic)

The following reaction is exothermic at constant pressure

N₂(g) + 3 H₂(g) → 2 NH₃(g)

Which of the following can be said about the reaction?

Shown below are system representations of three equilibrium mixtures for the interconversions of B molecules to X, B molecules to Y, and B molecules to Z. The molecules of B are shown as yellow spheres while molecules of X, Y, or Z are green spheres. Determine the sign of ΔG° for each case.