Given the following reaction: CO (g) + Cl2 (g) → COCl2 (g). Determine the orders for CO and Cl2 and then write the rate law for this reaction. Then calculate the rate constant, k, and include the proper units. Show all your work and units.
Added by Muzan O.
Step 1
First, we need to determine the orders for CO and Cl2. The order of a reaction is determined by the stoichiometric coefficients in the balanced chemical equation. In this case, both CO and Cl2 have a coefficient of 1, so the reaction is first order with respect to Show more…
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The rate law for the reaction between $\mathrm{CO}(g)$ and $\mathrm{Cl}_{2}(g)$ to form phosgene, $\mathrm{Cl}_{2} \mathrm{CO}(g)$, described by $$ \mathrm{Cl}_{2}(g)+\mathrm{CO}(g) \rightarrow \mathrm{Cl}_{2} \mathrm{CO}(g) $$ is $$ \text { rate of reaction }=k\left[\mathrm{Cl}_{2}\right]^{3 / 2}[\mathrm{CO}] $$ Show that the following mechanism is consistent with this rate law (1) $\mathrm{Cl}_{2}(g) \frac{k_{\mathrm{l}}}{\mathrm{k}_{-1}} 2 \mathrm{Cl}(g) \quad$ (fast equilibrium) (2) $\mathrm{Cl}(g)+\mathrm{CO}(g) \frac{k_{4}}{\vec{k}_{-2}} \mathrm{ClCO}(g) \quad$ (fast equilibrium) (3) $\mathrm{ClCO}(g)+\mathrm{Cl}_{2}(g) \stackrel{k_{3}}{\longrightarrow} \mathrm{Cl}_{2} \mathrm{CO}(g)+\mathrm{Cl}(g) \quad$ (slow) Express $k$ in terms of the rate constants for the individual steps of the reaction mechanism.
The tabulated data were collected for this reaction: $$\mathrm{CH}_{3} \mathrm{Cl}(g)+3 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g)+3 \mathrm{HCl}(g)$$ Write an expression for the reaction rate law and calculate the value of the rate constant, $k$ . What is the overall order of the reaction?
The tabulated data were collected for this reaction: $$ \mathrm{CH}_{3} \mathrm{Cl}(g)+3 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g)+3 \mathrm{HCl}(g) $$ $$ \begin{array}{ccc} {\left[\mathrm{CH}_{3} \mathrm{Cl}\right](\mathrm{M})} & {\left[\mathrm{Cl}_{2}\right](\mathrm{M})} & \text { Initial Rate }(\mathrm{M} / \mathrm{s}) \\ \hline 0.050 & 0.050 & 0.014 \\ \hline 0.100 & 0.050 & 0.029 \\ \hline 0.100 & 0.100 & 0.041 \\ \hline 0.200 & 0.200 & 0.115 \\ \hline \end{array} $$ Write an expression for the reaction rate law and calculate the value of the rate constant, $k$. What is the overall order of the reaction?
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