EasyChemistryHigh School (11–12)The p-Block ElementsNumerical

Find the oxidation state of nitrogen in each species: N₂O, NO₂⁻, NO₃⁻, NH₄⁺, N₂H₄ and NH₂OH…

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Find the oxidation state of nitrogen in each species: $\text{N}_{2}\text{O}$ , $\text{NO}_{2}^{-}$ , $\text{NO}_{3}^{-}$ , $\text{NH}_{4}^{+}$ , $\text{N}_{2}\text{H}_{4}$ and $\text{NH}_{2}\text{OH}$ . Take oxygen as $-2$ and hydrogen as $+1$ . In $\text{N}_{2}\text{H}_{4}$ and $\text{NH}_{2}\text{OH}$ the two atoms of nitrogen, or the one atom of nitrogen, share the rest.

Need a reminder? The key ideaShow

Oxidation states of nitrogen run from $-3$ to $+5$ . Nitric acid is reduced to NO2 when concentrated and to NO, N2O or NH4+ when dilute. Count electrons: a metal atom that gives up $n$ electrons needs $n$ electrons to be taken by the nitrogen. At 273 K and 1 atm, 1 mol of gas fills 22.4 L. The Ostwald process gives 1 mol of HNO3 for each mole of NH3 at a full yield.

The worked solution

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← At 600 K the equilibrium constant of N₂ + 3H₂ ⇌ 2NH₃ is Kp = 4.43 × 10⁻³ bar⁻²…A plant burns 8.50 t of ammonia each day in the Ostwald process… →

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