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A balanced chemical equation represents a chemical reaction with the same number of atoms for each element on both the reactant and product sides. This ensures the conservation of mass. In the given exercise, the overall reaction from the Raschig process is:

aqt{NaOCl (aq) + 2 NH₃ (aq) → Na₂H₄ (aq) + NaCl (aq) + H₂O (l)}aqt
This means for every 1 mole of sodium hypochlorite (NaOCl) and 2 moles of ammonia (NH₃), we get 1 mole of hydrazine (N₂H₄), 1 mole of sodium chloride (NaCl), and 1 mole of water (H₂O). Balancing the equation involves making sure the same number of atoms for each element is present on both sides.

• Na: 1 atom on both sides
• O: 1 atom on both sides
• Cl: 1 atom on both sides
• N: 2 atoms on both sides
• H: 8 atoms on both sides

Balancing chemical equations is critical for accurate stoichiometric calculations, including percent atom economy.

Calculating molar masses involves summing the atomic masses of all atoms in a molecule. For instance, in the given equation:

• NaOCl: Na (23 g/mol) + O (16 g/mol) + Cl (35.5 g/mol) = 74.5 g/mol
• NH₃: 14 (N) + 3 * 1 (H) = 17 g/mol. Since there are 2 NH₃, we get 34 g/mol
• Nâ‚‚Hâ‚„: 2 * 14 (N) + 4 * 1 (H) = 32 g/mol
• NaCl: Na (23 g/mol) + Cl (35.5 g/mol) = 58.5 g/mol
• Hâ‚‚O: 2 * 1 (H) + 16 (O) = 18 g/mol

Using these molar mass values, we calculate the total molar mass of the reactants. It is 74.5 g/mol for NaOCl plus 34 g/mol for 2 NH₃, resulting in 108.5 g/mol. Molar mass calculations are pivotal in understanding the quantities of substances involved in reactions, which helps in analyzing efficiencies like atom economy.

Hydrazine (Nâ‚‚Hâ‚„) is a valuable compound used as rocket fuel due to its high energy content and the exothermic nature of its decomposition. Related to the given Raschig process equation:

aqt{NaOCl (aq) + 2 NH₃ (aq) → N₂H₄ (aq) + NaCl (aq) + H₂O (l)}aqt

Hydrazine's efficient production and combustion are vital in the chemical propulsion of rockets:

• High-energy output from its combustion
• Easy storage and handling compared to some alternative propellants
• Provides thrust necessary for rocket propulsion

The proficiency of hydrazine as a rocket fuel underscores why processes like the Raschig process are essential in rocket fuel chemistry. Understanding how this fuel is synthesized ensures its reliable and efficient use in aerospace applications.

The Raschig process is a key industrial method for synthesizing hydrazine (Nâ‚‚Hâ‚„). It involves a series of chemical reactions starting from ammonia and sodium hypochlorite. The given overall equation for the process is:

aqt{NaOCl (aq) + 2 NH₃ (aq) → N₂H₄ (aq) + NaCl (aq) + H₂O (l)}aqt

This three-step process includes:

• Reaction of NaOCl with NH₃ to form chloramine (NHâ‚‚Cl)
• Further reaction of NHâ‚‚Cl with NH₃ to form hydrazine (Nâ‚‚Hâ‚„)
• Generation of by-products like NaCl and Hâ‚‚O

The Raschig process ensures the efficient production of hydrazine, which is not only used as a rocket fuel but also in various industrial applications such as water treatment and polymerization processes. Mastering the Raschig process helps in optimizing the synthesis and yields of hydrazine, making it economically viable and environmentally friendly.