This question has multiple parts. Work all the parts to get the most points. The reaction \[ 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{NOCl}(g) \] was studied at \( -10^{\circ} \mathrm{C} \). The following results were obtained where \[ \text { Rate }=-\frac{\triangle\left[\mathrm{Cl}_{2}\right]}{\triangle t} \] \begin{tabular}{ccc} {\( [\mathrm{NO}]_{0} \)} & {\( \left[\mathrm{Cl}_{2}\right]_{0} \)} & Initial Rate \\ \( (\mathrm{mol} / \mathrm{L}) \) & \( (\mathrm{mol} / \mathrm{L}) \) & \( (\mathrm{mol} / \mathrm{L} \cdot \mathrm{min}) \) \\ 0.10 & 0.10 & 0.18 \\ 0.10 & 0.20 & 0.36 \\ 0.20 & 0.20 & 1.44 \end{tabular} a What is the rate law? ( Use \( k \) for the rate constant. ) Rate \( = \) \( \square \)
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The question provides experimental data for the reaction between NO and Cl2 to form NOCl and asks for the rate law of the reaction. The rate law is an equation that relates the rate of a reaction to the concentrations of the reactants and a rate constant (k). Show more…
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The reaction $$ 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NOCl}(g) $$ was studicd at $-10^{\circ} \mathrm{C}$. The following results were obtained, where $$ \text { Rate }=-\frac{d\left[\mathrm{Cl}_{2}\right]}{d t} $$ $$\begin{array}{ccc} &{\text { Initial Rate }} \\ [\mathrm{NO}]_{0}(\mathrm{mol} / \mathrm{L}) & \left[\mathrm{Cl}_{2}\right]_{0}(\mathrm{mol} / \mathrm{L}) & \left(\mathrm{mol} \mathrm{L}^{-1} \mathrm{min}^{-1}\right) \\ \hline 0.10 & 0.10 & 0.18 \\ 0.10 & 0.20 & 0.36 \\ 0.20 & 0.20 & 1.45 \end{array}$$ a. What is the rate law? b. What is the value of the rate constant?
Rate Laws from Experimental Data: Initial Rates Method. The reaction $$2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NOCl}(g)$$ was studied at $-10^{\circ} \mathrm{C}$. The following results were obtained where $$\text { Rate }=-\frac{\Delta\left[\mathrm{Cl}_{2}\right]}{\Delta t}$$ $$ \begin{array}{ccc} {[\mathrm{NO}]_{0}} & {\left[\mathrm{Cl}_{2}\right]_{0}} & \text { Initial Rate } \\ (\mathrm{mol} / \mathrm{L}) & (\mathrm{mol} / \mathrm{L}) & (\mathrm{mol} / \mathrm{L} \cdot \mathrm{min}) \\ 0.10 & 0.10 & 0.18 \\ 0.10 & 0.20 & 0.36 \\ 0.20 & 0.20 & 1.45 \end{array} $$ a. What is the rate law? b. What is the value of the rate constant?
The reaction described by the equation $$ 2 \mathrm{NOCl}(g) \rightarrow 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) $$ was studied at $400 \mathrm{~K}$, and the following data were collected: \begin{tabular}{ccc} \hline & & Initial rate of \\ Run & {$[\mathrm{NOCl}]_{0} / \mathrm{M}$} & formation of $\mathrm{Cl}_{2}(g) / \mathrm{M} \cdot \mathrm{s}^{-1}$ \\ \hline 1 & $0.25$ & $1.75 \times 10^{-6}$ \\ 2 & $0.42$ & $4.94 \times 10^{-6}$ \\ 3 & $0.65$ & $1.18 \times 10^{-5}$ \\ \hline \end{tabular} Determine the rate law and the value of the rate constant for the reaction.
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