As we discussed in class, although low temperatures favor the formation of ammonia in Haber process, in practice higher temperatures, on the order of 450 ◦C, are used. (a) Repeat the computation of the relative reaction extent that we did in the class (or just use the formula for reaction extent given in the notes) at T = 450 ◦C and constant overall pressure of 1 bar and 200 bar. Assume that the reaction enthalpy and entropy do not depend on the temperature. You will need to consult thermodynamic tables to determine the equilibrium constant at this temperature. (b) Instead of keeping the overall pressure constant, assume that the reaction occurs in a fixed-volume container (at const T). Assuming that 3/2 mol of H2 and 1/2 mol of N2 are mixed at T = 450 ◦Cand p = 200 bar, determine the reaction extent at equilibrium. Note that p will now depend on the reaction extent, hence the relation between the reaction extent and Kp must be re-derived.
As we discussed in class, although low temperatures favor the formation of ammonia in Haber process, in practice higher temperatures, on the order of 450 ◦C, are used. (a) Repeat the computation of the relative reaction extent that we did in the class (or just use the formula for reaction extent given in the notes) at T = 450 ◦C and constant overall pressure of 1 bar and 200 bar. Assume that the reaction enthalpy and entropy do not depend on the temperature. You will need to consult
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