The Haber Process is used to produce ammonia (NH_3) from nitrogen and hydrogen.
ID: 507506 • Letter: T
Question
The Haber Process is used to produce ammonia (NH_3) from nitrogen and hydrogen. This process was originally developed to produce ammonia for the production of explosives to be used by Germany in World War I. It has subsequently been used to produce ammonia for fertilizer. This reaction releases 92.2 kJ of energy for every mole of nitrogen consumed. N_2 + 3H_2 rightarrow 2NH_3 a. How much energy (answer in Joules) can be produced from the consumption of 5.000 times 10^2 kg of nitrogen? b. What is the theoretical yield of ammonia if 5.000 times 10^2 kg of nitrogen is allowed to react with excess hydrogen?Explanation / Answer
Ans. #A. Amount of nitrogen = 5.000 x 102 kg = 500 kg = 500000 g
Moles of N2 = Mass/ Molar mass
= 500000 g / (28.0 g/ mol)
= 17857.143 mol
Given, rate of energy production during the process = 92.2 kJ/ mol N2
Total energy produced = Rate of energy production x Moles of N2
= (92.2 kJ/ mol N2) x 17857.143 mol N2
= 1646428.5846 kJ
= 1646428584.6 J
= 1.646 x 109 J
#B. In balanced reaction, 1 mol N2 produces 2 mol ammonia.
Thus,
Theoretical moles of NH3 formed = 2 x Moles of N2 consumed
= 2 x 17857.143 mol
= 35714.286 mol
Theoretical mass of NH3 formed = Theoretical moles of NH3 x Molar mass
= 35714.286 mol x (17.03 g/ mol)
= 608214.29 g
= 608.21 kg
Thus, theoretical yield of NH3 = 608.21 kg
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