Difficult
The mechanism of reaction $2 \ NO + Cl_2 \rightarrow 2 \ NOCl$ is given as :
$(i) 2 NO \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} N_2 O _2$ (fast)
$(ii) N_2O_2 + Cl_2 \xrightarrow{K_3} 2 \ NOCl$ (slow)
The rate expression of the reaction will be :
$(i) 2 NO \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} N_2 O _2$ (fast)
$(ii) N_2O_2 + Cl_2 \xrightarrow{K_3} 2 \ NOCl$ (slow)
The rate expression of the reaction will be :
- A$r = K_1 K_2 [N_2O_2][Cl_2]$
- B$r = \frac{K_1 K_3}{K_2} [NO]^2 [Cl_2]$
- C$r = K_1 K_2 [Cl_2]$
- D$r = K_1 K_2 K_3 [NO] [Cl_2]$
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