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Chemistry

Give balanced equations for (1) & (2) by partial equation method, [steps are given below]

  1. Reaction of excess ammonia with chlorine – Ammonia as a reducing agent
    (a) Ammonia first reacts with chlorine to give hydrogen chloride and nitrogen.
    (b) Hydrogen chloride then further reacts with excess ammonia to give ammonium chloride.
  2. Oxidation of Lead [II] Sulphide by Ozone
    (a) Ozone first decomposes to give molecular oxygen & nascent oxygen.
    (b) Nascent oxygen then oxidizes lead [II] sulphide to lead [II] sulphate.

Chemical Equation

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Answer

1. Reaction of excess ammonia with chlorine – Ammonia as a reducing agent

2NH3+3Cl2⟶6HCl+N26NH3+6HCl⟶6NH4Cl8NH3+3Cl2⟶6NH4Cl+N2\begin{array}{l} 2\text{NH}3 + 3\text{Cl}2 \longrightarrow \cancel{6\text{HCl}} + \text{N}2 \ 6\text{NH}3 + \cancel{6\text{HCl}} \longrightarrow 6\text{NH}4\text{Cl} \ \hline 8\text{NH}3 + 3\text{Cl}2 \longrightarrow 6\text{NH}4\text{Cl} + \text{N}_2 \end{array}

2. Oxidation of Lead [II] Sulphide by Ozone

O3⟶O2+[O]×4PbS+4[O]⟶PbSO4PbS+4O3⟶PbSO4+4O2\begin{array}{l} \text{O}3 \longrightarrow \text{O}2 + \cancel{\text{[O]}} \times 4 \ \text{PbS} + \cancel{4\text{[O]}} \longrightarrow \text{PbSO}4 \ \hline \text{PbS} + 4\text{O}3 \longrightarrow \text{PbSO}4 + 4\text{O}2 \end{array}

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