320535 Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide
\({\text{2N}}{{\text{O}}_{{\text{(g)}}}}{\text{  +  }}{{\text{O}}_{\text{2}}}{\text{(g)}}\xrightarrow{{\text{K}}}{\text{2N}}{{\text{O}}_{{\text{2(g)}}}}\)
If the mechanism of reaction is
\({\text{NO  +  }}{{\text{O}}_{\text{2}}}\mathop  \rightleftharpoons \limits_{\text{K}} {{\text{N}}_{\text{3}}}{\text{( fast )}}{\mkern 1mu} {\text{N}}{{\text{O}}_{\text{3}}}{\text{  +  NO}}\xrightarrow{{{{\text{K}}_{\text{1}}}}}\)
\({\text{N}}{{\text{O}}_{\text{2}}}{\text{  +  N}}{{\text{O}}_{\text{2}}}{\text{(slow)}}\)
then rate law is

320536 The plot of \({{\rm{t}}_{{\rm{1/2}}}}\,\,{\rm{v/s}}\,{{\rm{[R]}}_{\rm{0}}}\) for a reaction is a straight-line parallel to \(x\)-axis. The unit for the rate constant of this reaction is

320537 The reaction, \({\rm{X + 2Y + Z}} \to {\rm{N}}\) occurs by the following mechanism

(i) \(X + Y \rightleftharpoons M\) very rapid equilibrium)

(ii) \({\rm{M + Z}} \to {\rm{O}}\) (slow) (iii) \({\rm{O + Y}} \to {\rm{N}}\) (very fast)

What is the rate law for this reaction?

320538 The reaction, \(X_{2}+Y_{2} \rightarrow 2 X Y\) occurs by the following mechanism

(i) \(X_{2} \rightleftharpoons 2 X\) (fast)

(ii) \(X+Y_{2} \rightarrow X Y+X\) (slow)

(iii) \(X+Y \rightarrow X Y\) (fast)
What is the order of the reaction?

320535 Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide
\({\text{2N}}{{\text{O}}_{{\text{(g)}}}}{\text{  +  }}{{\text{O}}_{\text{2}}}{\text{(g)}}\xrightarrow{{\text{K}}}{\text{2N}}{{\text{O}}_{{\text{2(g)}}}}\)
If the mechanism of reaction is
\({\text{NO  +  }}{{\text{O}}_{\text{2}}}\mathop  \rightleftharpoons \limits_{\text{K}} {{\text{N}}_{\text{3}}}{\text{( fast )}}{\mkern 1mu} {\text{N}}{{\text{O}}_{\text{3}}}{\text{  +  NO}}\xrightarrow{{{{\text{K}}_{\text{1}}}}}\)
\({\text{N}}{{\text{O}}_{\text{2}}}{\text{  +  N}}{{\text{O}}_{\text{2}}}{\text{(slow)}}\)
then rate law is

320536 The plot of \({{\rm{t}}_{{\rm{1/2}}}}\,\,{\rm{v/s}}\,{{\rm{[R]}}_{\rm{0}}}\) for a reaction is a straight-line parallel to \(x\)-axis. The unit for the rate constant of this reaction is

320537 The reaction, \({\rm{X + 2Y + Z}} \to {\rm{N}}\) occurs by the following mechanism

(i) \(X + Y \rightleftharpoons M\) very rapid equilibrium)

(ii) \({\rm{M + Z}} \to {\rm{O}}\) (slow) (iii) \({\rm{O + Y}} \to {\rm{N}}\) (very fast)

What is the rate law for this reaction?

320538 The reaction, \(X_{2}+Y_{2} \rightarrow 2 X Y\) occurs by the following mechanism

(i) \(X_{2} \rightleftharpoons 2 X\) (fast)

(ii) \(X+Y_{2} \rightarrow X Y+X\) (slow)

(iii) \(X+Y \rightarrow X Y\) (fast)
What is the order of the reaction?

320535 Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide
\({\text{2N}}{{\text{O}}_{{\text{(g)}}}}{\text{  +  }}{{\text{O}}_{\text{2}}}{\text{(g)}}\xrightarrow{{\text{K}}}{\text{2N}}{{\text{O}}_{{\text{2(g)}}}}\)
If the mechanism of reaction is
\({\text{NO  +  }}{{\text{O}}_{\text{2}}}\mathop  \rightleftharpoons \limits_{\text{K}} {{\text{N}}_{\text{3}}}{\text{( fast )}}{\mkern 1mu} {\text{N}}{{\text{O}}_{\text{3}}}{\text{  +  NO}}\xrightarrow{{{{\text{K}}_{\text{1}}}}}\)
\({\text{N}}{{\text{O}}_{\text{2}}}{\text{  +  N}}{{\text{O}}_{\text{2}}}{\text{(slow)}}\)
then rate law is

320536 The plot of \({{\rm{t}}_{{\rm{1/2}}}}\,\,{\rm{v/s}}\,{{\rm{[R]}}_{\rm{0}}}\) for a reaction is a straight-line parallel to \(x\)-axis. The unit for the rate constant of this reaction is

320537 The reaction, \({\rm{X + 2Y + Z}} \to {\rm{N}}\) occurs by the following mechanism

(i) \(X + Y \rightleftharpoons M\) very rapid equilibrium)

(ii) \({\rm{M + Z}} \to {\rm{O}}\) (slow) (iii) \({\rm{O + Y}} \to {\rm{N}}\) (very fast)

What is the rate law for this reaction?

320538 The reaction, \(X_{2}+Y_{2} \rightarrow 2 X Y\) occurs by the following mechanism

(i) \(X_{2} \rightleftharpoons 2 X\) (fast)

(ii) \(X+Y_{2} \rightarrow X Y+X\) (slow)

(iii) \(X+Y \rightarrow X Y\) (fast)
What is the order of the reaction?

320535 Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide
\({\text{2N}}{{\text{O}}_{{\text{(g)}}}}{\text{  +  }}{{\text{O}}_{\text{2}}}{\text{(g)}}\xrightarrow{{\text{K}}}{\text{2N}}{{\text{O}}_{{\text{2(g)}}}}\)
If the mechanism of reaction is
\({\text{NO  +  }}{{\text{O}}_{\text{2}}}\mathop  \rightleftharpoons \limits_{\text{K}} {{\text{N}}_{\text{3}}}{\text{( fast )}}{\mkern 1mu} {\text{N}}{{\text{O}}_{\text{3}}}{\text{  +  NO}}\xrightarrow{{{{\text{K}}_{\text{1}}}}}\)
\({\text{N}}{{\text{O}}_{\text{2}}}{\text{  +  N}}{{\text{O}}_{\text{2}}}{\text{(slow)}}\)
then rate law is

320536 The plot of \({{\rm{t}}_{{\rm{1/2}}}}\,\,{\rm{v/s}}\,{{\rm{[R]}}_{\rm{0}}}\) for a reaction is a straight-line parallel to \(x\)-axis. The unit for the rate constant of this reaction is

320537 The reaction, \({\rm{X + 2Y + Z}} \to {\rm{N}}\) occurs by the following mechanism

(i) \(X + Y \rightleftharpoons M\) very rapid equilibrium)

(ii) \({\rm{M + Z}} \to {\rm{O}}\) (slow) (iii) \({\rm{O + Y}} \to {\rm{N}}\) (very fast)

What is the rate law for this reaction?

320538 The reaction, \(X_{2}+Y_{2} \rightarrow 2 X Y\) occurs by the following mechanism

(i) \(X_{2} \rightleftharpoons 2 X\) (fast)

(ii) \(X+Y_{2} \rightarrow X Y+X\) (slow)

(iii) \(X+Y \rightarrow X Y\) (fast)
What is the order of the reaction?