In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitroge

Question

In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction is now the first step taken to make most of the world's fertilizer. Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 770. liters per second of dinitrogen are consumed when the reaction is run at 161·°C and 0.87 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. kg x10

Explanation / Answer

Ideal gas equation is

PV = nRT

n = PV/RT

= 0.87atm × 770L/0.082057(L atm/mol K) × 434.15K

= 18.804mol

18.804 mol of N2 consumed per second

Balanced equation of this reaction is

N2(g) + 3H2(g) <------>2NH3(g)

So, 1mole of N2 giving 2 mole of NH3

Therefore,

18.804mol of N2 give 2×18.804 = 37.608mole of NH3

Molar mass of NH3 = 17.031g/mol

Mass of produced per second = 17.031g/mol × 37.608mol =640.50g = 0.64050kg

Therefore,

Rate of production of ammonia = 0.641kg/s

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