For the gas-phase reaction A = 2B operated at 1.0 bar: Initially, the reactor contains only A, at 1.0 mol. a. Prove that the reaction coordinate (moles of A consumed) equals the following: (see attactched image) b. Make a plot of the reaction coordinate versus temperature between 200 and 400 K for exothermic reaction conditions, making use of the van’t Hoff Equation. Data: Ka = 5.0 at 298 K, ΔHrxn0 = -50.0 kJ mol-1. Neglect the ΔCp term. c. Repeat Part b for endothermic conditions. Ka = 5.0 at 298 K, ΔHrxn0 = +50.0 kJ mol-1. Neglect the ΔCp term.
For the gas-phase reaction A = 2B operated at 1.0 bar: Initially, the reactor contains only A, at 1.0 mol.
a. Prove that the reaction coordinate (moles of A consumed) equals the following:
(see attactched image)
b. Make a plot of the reaction coordinate versus temperature between 200 and 400 K for exothermic reaction conditions, making use of the van’t Hoff Equation. Data: Ka = 5.0 at 298 K, ΔHrxn0 = -50.0 kJ mol-1. Neglect the ΔCp term.
c. Repeat Part b for endothermic conditions. Ka = 5.0 at 298 K, ΔHrxn0 = +50.0 kJ mol-1. Neglect the ΔCp term.
d. If the reaction described in part b (i.e., exothermic conditions) were operated in a simple batch reactor, would the reaction mixture’s temperature increase, decrease, or remain constant as the reaction progressed? To maximize conversion, would you recommend that heat be added to, or removed from, the reactor?
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