At the Nangal fertilizer plant in Punjab, hydrogen is produced by the electrolysis of water. The hyd — Electrochemistry Chemistry Question
Question
At the Nangal fertilizer plant in Punjab, hydrogen is produced by the electrolysis of water. The hydrogen is used for the production of ammonia and nitric acid (by the oxidation of ammonia). If the average production of ammonium nitrate is 1152 kg/day, the daily consumption of electricity (in A /day) is
💡 Solution & Explanation
Molar mass of NH4NO3 = 80 g/mol. Moles of NH4NO3 = 1152 × 1000 / 80 = 14400 mol/day. Producing 1 mole of NH4NO3 (which contains NH4+ and NO3-) requires 2 moles of NH3 overall. Total NH3 required = 28800 mol/day. From N2 + 3H2 -> 2NH3, 1 mole of NH3 needs 1.5 moles of H2. Total H2 required = 1.5 × 28800 = 43200 mol/day. Electrolysis of water (2H^+ + 2e^– -> H2) needs 2 F per mole of H2. Charge required = 43200 × 2 = 86400 F/day. Current I = Total Charge / Time = (86400 × 96500 C) / (24 × 3600 s) = 86400 × 96500 / 86400 = 96500 A. Therefore, correct answer is A.