Irreversible reaction

Hydrazine nitrosated to ammonia and nitrous oxide (selectivity loss)

N2H4+CH3NO2N2O+NH3+CH4O

Direction
Irreversible
Processes
1
Stated as
Rate law
Heat of reaction
ΔH = -178,500 kJ/kmol (one process)
Element balance
Checked: balances
As the processes state itStoichiometry, conversions, heats of reaction and catalyst windows are taken from each process's files with their provenance. The build checks only that each process's equation balances in every element, from the process's own component formulas; it does not check the numbers. A process's design maturity applies to them.

Species

SpeciesNameCASRoleCoefficient
N2H4Hydrazine302-01-2reactant-1
CH3NO2Methyl nitrite624-91-9reactant-1
N2ONitrous oxide10024-97-2product1
NH3Ammonia7664-41-7product1
CH4OMethanol67-56-1product1

In the processes

  • Sodium azide by the hydrazine / methyl nitrite route, batch, with precipitation from the reaction liquor (670 t/a)Concept · not reviewed

    SIDE · Hydrazine nitrosated to ammonia and nitrous oxide (selectivity loss)N2H4 + CH3ONO → N2O + NH3 + CH3OH

    Stated as
    Rate law
    Phase
    liquid
    Element balance
    Balances in every element
    Heat of reaction
    ΔH = -178,500 kJ/kmol at 298.15 K, as written (assumed: 82.574 - 45.558 - 238.4 - 285.825 - (-242.57 - 66.1) kJ/mol: N2H4.H2O(l) + CH3ONO(g) -> N2O(g) + NH3(g) + CH3OH(l) + H2O(l), pure-substance standard states (chemicals: ATcT, CRC); N2O and NH3 formed as gases, as they leave by the vent (core ADR 0054, D-005))
    Rate law
    basis: volume; driving: concentration; form: power_law; k: {"A":"5.3684e5","Ea":60000}; orders: {"MEONO":1,"N2H4":1}; temperature range: 293.15 – 323.15 (assumed: ASSUMED: AZ's rate law at 0.05/0.95 of its constant, the patent's 95 % selectivity on hydrazine (D-005))

Sources

What the processes cite for this reaction, each source once: for the reaction itself, its conversion, its heat of reaction or its catalyst. As the processes write them; DOIs, US patent numbers and web addresses are linked.

  1. US 5 208 002 A Example 1 (NaOH consumed equals the NaN3 formed; about 5 % of the hydrazine consumed gives no azide); Perrott, Stedman, Uysal, J. Chem. Soc. Dalton Trans. 1976, 2058 (ammonia and N2O as the low-acidity products of hydrazine nitrosation; abstract seen in a search, not read)

    For the reaction · cited by Sodium azide by the hydrazine / methyl nitrite route, batch, with precipitation from the reaction liquor (670 t/a)

  2. 82.574 - 45.558 - 238.4 - 285.825 - (-242.57 - 66.1) kJ/mol: N2H4.H2O(l) + CH3ONO(g) -> N2O(g) + NH3(g) + CH3OH(l) + H2O(l), pure-substance standard states (chemicals: ATcT, CRC); N2O and NH3 formed as gases, as they leave by the vent (core ADR 0054, D-005)

    For the heat of reaction · cited by Sodium azide by the hydrazine / methyl nitrite route, batch, with precipitation from the reaction liquor (670 t/a)