The elementary liquid-phase series reaction A→k1B→k2C is carried out in a 500-dm³ batch reactor. The initial concentration of A is 1.6 mol/dm³. The desired product is B, and separation of the undesired product C is very difficult and costly. Because the reaction is carried out at a relatively high temperature, the reaction is easily quenched.
a. Plot and analyze the concentrations of A, B, and C as a function of time. Assume that each reaction is irreversible, with k₁ = 0.4 h^–1 and k₂ = 0.01 h^–1.
b. Plot and analyze the concentrations of A, B, and C as a function of time when the first reaction is reversible, with k_–1 = 0.3 h^–1.
c. Plot and analyze the concentrations of A, B, and C as a function of time for the case where both reactions are reversible, with k_–2 = 0.005 h^–1.
d. Vary k₁, k₂, k_–1, and k_–2. Explain the consequence of k₁ > 100 and k₂ < 0.1 with k_–1 = k_–2 = 0 and with k_–2 = 1, k_–1 = 0, and k_–2 = 0.25.