🤓 Based on our data, we think this question is relevant for Professor Combrink's class at TAMIU.

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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Based on our data, we think this problem is relevant for Professor Combrink's class at TAMIU.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.