P3-2 (a) Example 3-1. Make a plot of k versus T and In k versus (1/7) for E = 240 kJ/mol, for E = 60 kJ/mol. (1) Write a couple of sentences describ- ing 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/dm?? (d) Example 3-4. What is the smallest value of n = (NB0/Nx0) 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 (11-r) as a function of X up to X = 0.99. What did you find? (1) Example 3-6. Why is the equilibrium conversion lower for the batch sys- tem than the flow system? Will this always be the case for constant vol- ume batch systems? For the case in which the total concentration Crois to remain constant as the inerts are varied. plot the equilibrium conver- sion as a function of mole fraction of inerts for both a PFR and a con- stant-volume batch reactor. The pressure and temperature are constant at 2 atm and 340 K. Only N.O, and inert I are to be fed. (g) Collision Theory- Professional Reference Shelf. Make an outline of the steps that were used to derive -A = Ae HRTCCB (h) The rate law for the reaction (2A + B +C) is - a = kac Co with kA = 25(dm mol/s. What are kg and ke? (i) At low temperatures the rate law for the reaction - A = ACC. If the reaction is reversible at high temperatures, what is the rate law? (44+%B-C) is