One day at the fertilizer factory, your boss Mr. Haber comes to you with a problem. The process used by the factory to produce ammonia,the raw material for your fertilizer, is just not optimized. He would like to modify the conditions to achieve a better yield of ammonia in the shortest possible time, and asks you to suggest One day at the fertilizer factory, your boss Mr. Haber comes to you with a problem. The process used by the factory to produce ammonia,the raw material for your fertilizer, is just not optimized. He would like to modify the conditions to achieve a better yield of ammonia in the shortest possible time, and asks you to suggest some changes. Consider the following equation,describing the process used by your factory:
N2(g) + 3 H2(g) ---> 2NH3(g) ΔHrxn=-92.4 KJ/mol
How will each of the following affect the yeild ofNH3,the equilibrium constant (K), the rate of the reaction and the value of the rate constant (k)? Assume constant pressure unless otherwise indicated, and that the rate law israte=k[N2]m[H2]n, whereboth m and n are greater than 0.
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Yield ofNH3 Equilibrium constant(K) Rate of rxn Rate constant(k)
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adding N2
removing H2
removing NH3
increasing
pressure
increasing
temp
adding catalyst
What is your recommendation to MR. Harber?