Determine the rate equation, the rate constant, and the overall order for this reaction

2NOCl_{(g)} ⟶ 2NO_{(g) }+ Cl_{2 (g)}

Step 1. Calculate the order

$\overline{)\frac{{\mathbf{rate}}_{\mathbf{2}}}{{\mathbf{rate}}_{\mathbf{1}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{{\left[\mathrm{NOCl}\right]}^{\mathbf{x}}\mathbf{}\mathbf{of}\mathbf{}{\mathbf{rate}}_{\mathbf{2}}}{{\left[\mathrm{NOCl}\right]}^{\mathbf{x}}\mathbf{}\mathbf{of}\mathbf{}{\mathbf{rate}}_{\mathbf{1}}}}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{8}\mathbf{.}\mathbf{0}\mathbf{}\mathbf{\times}\mathbf{}{\mathbf{10}}^{\mathbf{-}\mathbf{10}}}{\mathbf{3}\mathbf{.}\mathbf{2}\mathbf{}\mathbf{\times}\mathbf{}{\mathbf{10}}^{\mathbf{-}\mathbf{9}}}\mathbf{}\mathbf{=}\mathbf{}\frac{{\left[\mathbf{0}\mathbf{.}\mathbf{20}\right]}^{\mathbf{x}}}{{[0.10]}^{\mathbf{x}}}\phantom{\rule{0ex}{0ex}}\mathbf{4}\mathbf{}\mathbf{=}\mathbf{}{\left[2\right]}^{\mathbf{x}}$

2 raised to 2 = 4

x = 2 → 2nd order

**Since there is only 1 reactant, the overall order is 2nd order**

Step 2. Setup rate law

**The rate law of the reaction is: rate =k[NOCl]**^{2}

Nitrosyl chloride, NOCl, decomposes to NO and Cl_{2}.

2NOCl_{(g)} ⟶ 2NO_{(g) }+ Cl_{2 (g)}

Determine the rate equation, the rate constant, and the overall order for this reaction from the following data:

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