Identify the molecularity and write the rate law for each of the following elementary reactions:
(a) $N O_{(g)} + O_{3 (g)} ⟶ N O_{3 (g)} + O_{(g)}$
(b) $H_{2} I_{(g)} + I_{(g)} ⟶ 2 H I_{(g)}$
(c) $C l_{(g)} + C l_{(g)} + N_{2 (g)} ⟶ C l_{2 (g)} + N_{2 (g)}$

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Solution

Molecularity is no. of molecules that come together to react in an elementary reaction is equal to sum of stoichiometric coefficients of reactants in elementary reaction.
(a) $N O + O_{3} ⟶ {N O}_{3} + O \Rightarrow$ $= 2$
(b) $H_{2} I + I ⟶ 2 H I \Rightarrow$ Molecularity $= 2$
(c) ${C l}_{(g)} + {C l}_{(g)} + N_{2 (g)} ⟶ {C l}_{2 (g)} + N_{2 (g)} \Rightarrow$ Molecularity $= 3$

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Similar questions

C l_{(g)} + O_{3 (g)} \to C l O_{(g)} + O_{2 (g)}

C l O_{(g)} + O_{(g)} \to C l_{(g)} + O_{2 (g)}

C l_{(g)} + O_{3 (g)} \to C l O_{(g)} + O_{2 (g)}

C l O_{(g)} + O_{(g)} \to C l_{(g)} + O_{2 (g)}

S t e p 1 : N_{2} O_{(g)} \to N_{2 (g)} + O_{(g)}

S t e p 2 : N_{2} O_{(g)} + O_{(g)} \to N_{2 (g)} + O_{2 (g)}

O_{3}

O_{3} (g) + C l (g) ⟶ O_{2} (g) + C l O (g);

k_{1} = 5.2 \times 10^{9} L {m o l}^{- 1} {s e c}^{- 1}

C l O (g) + O (g) ⟶ C l (g) + O_{2} (g);

k_{2} = 2.6 \times 10^{10} L {m o l}^{- 1} {s e c}^{- 1}

O_{3} (g) + O (g) ⟶ 2 O_{2} (g)

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