6. The Haber Process is a large scale industrial process of producing ammonia fr

Question

6. The Haber Process is a large scale industrial process of producing ammonia from nitrogen and hydrogen. The relevant reaction is: N2 (g) + 3 H2 (g) 2 NH3 (g) a. If a Haber plant is consuming hydrogen at a rate of 215 moles per hour, what is the rate of production of ammonia, in moles per hour? b. If the plant operates 24 hours per day, and the plant manager wants the product yield to be 5.0 metric tons of ammonia per day, what would be the required rate of injection of nitrogen, in moles per hour.

Explanation / Answer

a)

In the balanced reaction, 3 moles of H2 yields 2 moles of ammionia

Rate of Production of ammonia = Rate of consumption of H2 * 2/3 = 215 moles/hr * 2/3 = 143.33 moles/hour

b)

Amount of ammonia = 5 metric tonnes = 5 * 10^6 g

Number of moles of ammonia = Mass/molar mass = 5 * 10^6/17 = 2.941 * 10^5 moles

Rate of moles ammonia needs to be produced /hour * 24 hour = 2.941 * 10^5

Rate of moles of ammonia needs to be produced = 12254.90 moles/hour

One mole of N2 gives 2 moles of NH3

Rate of injection of nitrogen = 1/2 * 12254.90 mol/hour = 6127.45 mol/hr

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