A mixture of one part nitrogen and three parts hydrogen molecules is heated to a

Question

A mixture of one part nitrogen and three parts hydrogen molecules is heated to a temperature of 500 0 C (the reaction of nitrogen “fixation,” N 2 + 3H 2 ? 2NH 3 puts the nitrogen in a form that plants can utilize to synthesize amino acids and other important molecules). A mixture of one part nitrogen and three parts hydrogen molecules is heated to a temperature of 500 oC (the reaction of nitrogen "fixation," N2+3H2 2NH3 puts the nitrogen in a form that plants can utilize to synthesize amino acids and other important molecules). 1. Write down the chemical equilibrium condition. 2. Derive the corresponding "aw of mass action" expressing ratios of powers of con- centrations as a function of the temperature. (Use TnN2c 28rnpC2, m112 2mpC2, mNH17mpe2 -, where mp is the proton mass, where I is the energy freed (per ammo- nia molecule) when a nitrogen and three hydrogen molecules form two ammonia molecules 3. Suppose the final total pressure (the total pressure is the sum of partial pressures of the nitrogen, hydrogen, and ammonia) is 400 atm. Pretend that the gases stll behave as ideal despite the high pressure. What fraction of the nitrogen molecules is converted to ammonia, then? (Write your answer as an equation expressing a function of the ratio nNHs/nN2 as a number times e.) High pressures are required in order to produce a large enough fraction of ammonia can you explain qualitatively why?

Explanation / Answer

1)   N2(g) + 3H2(g) 2NH3(g) + Heat ..(I)

Keq =   (conc of NH3)^2/(conc of N2)^1* (conc of H2)^2

2) Keq = (17mpc^2)^2/(28 mc^2* (2mpc^2)^3 - I

3) we get lesser percentage of N2 gas

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