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. Gibbs free energy of formation of NH3 at 450 ◦C is 25.72 kJ mol−1 . (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 ◦C and 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. Gibbs free energy of formation of NH3 at 450 ◦C
is 25.72 kJ mol−1
. (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 ◦C and 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.
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