Researchers study the thermal dissociation of diatomic phosphorus according to the equilibrium reaction
P2(g)⇌2P(g)
In a series of experiments at a fixed temperature, different initial amounts of P2(g) are sealed in identical, rigid containers of equal volume. For each experiment, the total pressure and the partial pressure of atomic phosphorus, P(g), are measured after the system reaches equilibrium.
(a) Outline a step-by-step procedure, using only the experimental measurements described above, to calculate the numerical value of the equilibrium constant Kc for one of the experiments.
(b) Explain why, at this fixed temperature, the value of Kc you calculate in part (a) would be the same no matter which initial pressure of P2(g) is chosen.
(c) Suppose the dissociation reaction is endothermic. Predict how the magnitude of Kc will change if the temperature is increased, and justify your prediction in terms of thermodynamic principles.