2) Give the molecularity and write the rate law for each of the following elementary reactions
a. $\mathrm{O} 3(\mathrm{~g})+\mathrm{Cl}(\mathrm{g}) \rightarrow \mathrm{O} 2(\mathrm{~g})+\mathrm{ClO}(\mathrm{g})$
b. $\mathrm{NO} 2(\mathrm{~g}) \rightarrow \mathrm{NO}(\mathrm{g})+\mathrm{O}(\mathrm{g})$
c. $\mathrm{ClO}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \rightarrow \mathrm{O} 2(\mathrm{~g})+\mathrm{Cl}(\mathrm{g})$
d. $\mathrm{Cl}(\mathrm{g})+\mathrm{Cl}(\mathrm{g})+N 2(\mathrm{~g}) \rightarrow \mathrm{Cl} 2(\mathrm{~g})+N 2(g)$
[molecularity; 2, 1, 2, 3]

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Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Determine molecularity and rate law for reaction a**: Molecularity refers to the number of molecules that come together to react in an elementary step. The molecularity of the given reaction a is 2, as there are two reactants, O3 and Cl. The rate law for an elementary reaction can be directly written from the stoichiometry of the reactants. ‖ ‖ 2 ⋮ **Write the rate law for reaction a**: The rate law for reaction a, based on its molecularity, is given by the expression $rate = k[O_3][Cl]$, where $k$ is the rate constant, and $[O_3]$ and $[Cl]$ are the concentrations of ozone and chlorine, respectively. ‖ ∻a Answer∻ ⚹ Molecularity: 2, Rate Law: $rate = k[O_3][Cl]$ ⚹ ‖ 3 ⋮ **Determine molecularity and rate law for reaction b**: The molecularity of reaction b is 1, as there is only one reactant, NO2. The rate law for a unimolecular reaction is based on the concentration of the single reactant. ‖ ‖ 4 ⋮ **Write the rate law for reaction b**: The rate law for reaction b is $rate = k[NO_2]$, where $k$ is the rate constant, and $[NO_2]$ is the concentration of nitrogen dioxide. ‖ ∻b Answer∻ ⚹ Molecularity: 1, Rate Law: $rate = k[NO_2]$ ⚹ ‖ 5 ⋮ **Determine molecularity and rate law for reaction c**: The molecularity of reaction c is 2, as there are two reactants, ClO and O. ‖ ‖ 6 ⋮ **Write the rate law for reaction c**: The rate law for reaction c is $rate = k[ClO][O]$, where $k$ is the rate constant, and $[ClO]$ and $[O]$ are the concentrations of chlorine monoxide and oxygen atom, respectively. ‖ ∻c Answer∻ ⚹ Molecularity: 2, Rate Law: $rate = k[ClO][O]$ ⚹ ‖ 7 ⋮ **Determine molecularity and rate law for reaction d**: The molecularity of reaction d is 3, as there are three reactants, two Cl atoms and one N2 molecule. ‖ ‖ 8 ⋮ **Write the rate law for reaction d**: The rate law for reaction d is $rate = k[Cl]^2[N_2]$, where $k$ is the rate constant, $[Cl]$ is the concentration of chlorine atoms, and $[N_2]$ is the concentration of nitrogen gas. ‖ ∻d Answer∻ ⚹ Molecularity: 3, Rate Law: $rate = k[Cl]^2[N_2]$ ⚹ ∻Key Concept∻ ⚹ Molecularity is the number of reactant molecules involved in an elementary step, and the rate law for an elementary reaction can be written from the stoichiometry of the reactants. ⚹ ∻Explanation∻ ⚹ The molecularity is determined by counting the number of reactant species in the elementary reaction, and the rate law is derived by combining the concentrations of the reactants raised to the power of their stoichiometric coefficients. ⚹◊What is the relationship between molecularity and the rate law of an elementary reaction in Chemistry?⍭ Generate me a similar question◊

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