The half-life of 2nd order reaction can be calculated as:

$\overline{){{\mathbf{t}}}_{\mathbf{1}\mathbf{/}\mathbf{2}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{1}}{\mathbf{k}{\left[\mathrm{NOCl}\right]}_{\mathbf{0}}}}\phantom{\rule{0ex}{0ex}}{\mathbf{t}}_{\mathbf{1}\mathbf{/}\mathbf{2}}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{1}}{(8x{10}^{-8}{M}^{-1}{s}^{-1})[0.15M]}$

What is the half-life for the decomposition of NOCl when the concentration of NOCl is 0.15 M? The rate constant for this second-order reaction is 8.0 × 10^{−8} L/mol/s.

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