(a) Example 3–1. Make a plot of k versus T and In k versus (1 IT) for E = 240 kJ/mol, for...

(a) Example 3–1. Make a plot of k versus T and In k versus (1 IT) for E = 240 kJ/mol, for E = 60 kJ/mol. (1) Write a couple of sentences describing what you find. (2) Next write a paragraph describing the activation energy, how it affects chemical reaction rates, and what its origins are?

(b) Example 3–2. Would the example be correct if water was considered an inert?

(c) Example 3–3. How would the answer change if the initial concentration or glyceryl stearate were 3 mol/dm3?

(d) Example 3–4. What is the smallest value of for which the concentration of B will not become the limiting reactant?

(e) Example 3–5. Under what conditions will the concentration of the inert nitrogen be constant? Plot Equation (E3-5.2) in terms of (1/—rA) as a function of X up to X = 0.99. What did you find?

(f) Example 3–6. Why is the equilibrium conversion lower for the batch system than the flow system? Will this always be the case for constant volume batch systems? For the case in which the total concentration C70 is to remain constant as the inerts are varied, plot the equilibrium conversion as a function of mole fraction of inerts for both a PFR and a constant-volume batch reactor. The pressure and temperature are constant at 2 atm and 340 K. Only N2O4 and inert I are to be fed.

(g) Collision Theory—Professional Reference Shelf. Make an outline of the steps that were used to derive

(h) The rate law for the reaction. What are kB and What are KB and Kc?

(i) At low temperatures the rate law for the reaction is If the reaction is reversible at high temperatures, what is the rate law?