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The proposed mechanism for a reaction is: A_(g)+B_(g) X_(g)(Fast) X_(g) +C_(…

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Wize University Chemistry Textbook > Kinetics

Reaction Mechanisms

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The proposed mechanism for a reaction is:

A(g)+B(g)↔X(g)(Fast)A_{(g)}+B_{(g)} \leftrightarrow X_{(g)}(Fast)
X(g)+C(g)↔Y(g)(Slow)X_{(g)} +C_{(g)}\leftrightarrow Y_{(g)}(Slow)
Y(g)→D(g)(Fast)Y_{(g)} \to D_{(g)}(Fast)
  1. What is the overall reaction?
  2. Identify the intermediates, if any.
More Reaction Mechanisms Questions:
The decomposition of ozone to oxygen gas can also occur in the presence of chlorine atoms. A proposed mechanism for this exothermic reaction is as follows:
Cℓ(g)+O3(g)→CℓO(g)+O2(g)slowO3(g)→O(g)+O2(g)fastCℓO(g)+O(g)→Cℓ(g)+O2(g)fast\begin{aligned}&C\ell(g)+O_3(g)\rightarrow C\ell O(g)+O_2(g)&slow\\ &O_3(g)\rightarrow O(g)+O_2(g)&fast \\&C\ell O(g)+O(g)\rightarrow C\ell(g)+O_2(g)&fast\end{aligned}
Which of these statements about this reaction is true?
The decomposition of ozone to oxygen gas can also occur in the presence of chlorine atoms. A proposed mechanism for this exothermic reaction is as follows:
Cℓ(g)+O3(g)→CℓO(g)+O2(g)slowO3(g)→O(g)+O2(g)fastCℓO(g)+O(g)→Cℓ(g)+O2(g)fast\begin{aligned}&C\ell(g)+O_3(g)\rightarrow C\ell O(g)+O_2(g)&slow\\ &O_3(g)\rightarrow O(g)+O_2(g)&fast \\&C\ell O(g)+O(g)\rightarrow C\ell(g)+O_2(g)&fast\end{aligned}
Which of these statements about this reaction is true?
A proposed mechanism for the reaction of NO2 with CO is shown below. Which of the given rate laws would accurately describe a reaction with this mechanism?
NO2(g)+NO2(g)→NO3(g)+NO(g)slowNO3(g)+CO(g)→NO2(g)+CO2(g)fastNO2(g)+CO(g)→NO(g)+CO2(g)overall\def\arraystretch{1.5} \begin{array}{cc} NO_2(g)+NO_2(g)\to NO_3(g)+NO(g) & slow \\ NO_3(g)+CO(g)\to NO_2 (g) +CO_2 (g) & fast \\ \hline NO_2(g)+CO(g)\to NO(g)+CO_2(g) & overall \end{array}
Practice: Reaction Mechanisms
For the reaction:
2NOCl(g)⟶2NO(g)+Cl2(g)Rateexp=k[NOCl]22NOCl(g)⟶2NO(g)+Cl_2 (g)\qquad Rate_{exp}=k[NOCl]^2
The following three mechanisms have been proposed :
Rate Laws: Reaction Mechanisms
For the reaction:
2NOCl(g)⟶2NO(g)+Cl2(g)Rateexp=k[NOCl]22NOCl(g)⟶2NO(g)+Cl_2 (g)\qquad Rate_{exp}=k[NOCl]^2
The following three mechanisms have been proposed :
Collision Theory: Ozone
The decomposition of ozone to oxygen gas can also occur in the presence of chlorine atoms. A proposed mechanism for this exothermic reaction is as follows:
Cℓ(g)+O3(g)→CℓO(g)+O2(g)slowO3(g)→O(g)+O2(g)fastCℓO(g)+O(g)→Cℓ(g)+O2(g)fast\begin{aligned}&C\ell(g)+O_3(g)\rightarrow C\ell O(g)+O_2(g)&slow\\ &O_3(g)\rightarrow O(g)+O_2(g)&fast \\&C\ell O(g)+O(g)\rightarrow C\ell(g)+O_2(g)&fast\end{aligned}
Which of these statements about this reaction is true?
A proposed mechanism for the reaction of NO2 with CO is shown below. Which of the given rate laws would accurately describe a reaction with this mechanism?
NO2(g)+NO2(g)→NO3(g)+NO(g)slowNO3(g)+CO(g)→NO2(g)+CO2(g)fastNO2(g)+CO(g)→NO(g)+CO2(g)overall\def\arraystretch{1.5} \begin{array}{cc} NO_2(g)+NO_2(g)\to NO_3(g)+NO(g) & slow \\ NO_3(g)+CO(g)\to NO_2 (g) +CO_2 (g) & fast \\ \hline NO_2(g)+CO(g)\to NO(g)+CO_2(g) & overall \end{array}
Reaction mechanisms: Rate law
The rate law for the overall reaction A + 2B → E was experimentally determined to be: Rate = k[A]2[B]
Which of these proposed mechanisms could explain this observed rate law?
Hydrogen spontaneously decomposes into two hydrogen atom radicals. One of these radicals reacts with an equivalent of fluorine gas to form one equivalent of HF and one fluorine atom. This fluorine atom reacts with a hydrogen atom to form another equivalent of HF. Write the mechanism of this reaction as series of elementary steps. Assign the molecularity of each step and write the overall reaction.
Collision Theory: Molecularity
Hydrogen spontaneously decomposes into two hydrogen atom radicals. One of these radicals reacts with an equivalent of fluorine gas to form one equivalent of HF and one fluorine atom. This fluorine atom reacts with a hydrogen atom to form another equivalent of HF. Write the mechanism of this reaction as series of elementary steps. Assign the molecularity of each step and write the overall reaction.