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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Similar Questions
$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.
By giving three examples,explain whether the exponents of the concentration terms in a rate law are the same as their stoichiometric coefficients in the balanced chemical reaction.
Difficult
View SolutionThe rate law for the reaction $2 NO_{(g)} + O_{2(g)} \longrightarrow 2 NO_{2(g)}$ is $\text{rate} = k[NO]^2[O_2]$. Which of the following statements is correct?
In a multistep reaction,the overall rate of reaction is equal to the
For the reaction $A + 2B \rightarrow \text{Product } (P)$,the rate law is given by $\frac{d[P]}{dt} = K[A]^2[B]$. If $[A]$ is taken in large excess,what will be the order of the reaction?
Medium
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