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

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answer is 6.

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Detailed Solution

$2 {NH}_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g)$
$rate = k | {NH}_{3}]$
$Rate = \frac{1}{3} \frac{d [H_{2}]}{d t}$
$\frac{d [H_{2}]}{dt} = 3 \times Rate \frac{d [H_{2}]}{dt} = 3 x 2 = 6$

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