# The rate of decomposition of  ${\mathrm{NH}}_{3}\left(\mathrm{g}\right)$ at 10 atm on platinum surface is zero order. What is rate of formation (in M  ${\mathrm{min}}^{-1}$) of ${\mathrm{H}}_{2}\left(\mathrm{g}\right)$ , if rate constant of reaction $2{\mathrm{NH}}_{{3}_{\left(\mathrm{g}\right)}}\to {\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)$  is 2.0 M ${\mathrm{min}}^{-1}$  ?

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### Solution:

$2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)⇌{\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)$
$\mathrm{rate}=\mathrm{k}|{\mathrm{NH}}_{3}\right]$
$\mathrm{Rate}=\frac{1}{3}\frac{\mathrm{d}\left[{\mathrm{H}}_{2}\right]}{dt}$

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