In the production of ammonia (NH3) by the Haber-Bosch process, calculate the mass of nitrogen gas (N2) required to produce 1 ton (1,000 kg) of ammonia.
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The balanced chemical equation for the production of ammonia (NH3) from nitrogen gas (N2) is:
N2 + 3H2 -> 2NH3
From this equation, we can see that 1 mole of N2 reacts to produce 2 moles of NH3. The molar mass of N2 is 28 g/mol.
To calculate the mass of nitrogen gas required to produce 1 ton (1,000 kg) of ammonia, we need to convert the given mass into moles.
1 ton (1,000 kg) = 1,000,000 grams
Number of moles of N2 = (mass of N2 / molar mass of N2) = (1,000,000 g / 28 g/mol) = 35,714.3 moles
Since 1 mole of N2 reacts to produce 2 moles of NH3, the number of moles of NH3 produced will be twice the number of moles of N2.
Number of moles of NH3 = 2 * 35,714.3 moles = 71,428.6 moles
To convert the number of moles of NH3 back into grams, we need to multiply by the molar mass of NH3.
The molar mass of NH3 is 17 g/mol.
Mass of NH3 = number of moles of NH3 * molar mass of NH3 = 71,428.6 moles * 17 g/mol = 1,214,285.7 grams
Therefore, the mass of nitrogen gas required to produce 1 ton (1,000 kg) of ammonia is approximately 1,214,286 grams or 1,214.286 kg.
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