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Zero Order Reaction

For a zero or...

Question

For a zero order chemical reaction,
$2 N H_{3} (g) \to N_{2} (g) + 3 H_{2} (g)$
rate of reaction $= 0.1$ atm/sec. Initially only $N H_{3}$ is present and its pressure $= 3$ atm. Calculate total pressure at $t = 10$ sec.

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Solution

For zero order reaction,

rate = rate constant $k$

& $[A] = - k t + [A_{o}]$

$(R a t e = k [A]^{^0})$

Given ${2 N H_{3}}_{(g)} ⟶ {N_{2}}_{(g)} + {3 H_{2}}_{(g)}$

$k = r a t e = 0.1 a t m$

$\Rightarrow [N H_{3}] = 3 a t m, t = 0,$
$\Rightarrow [N_{2}] = x$
$\Rightarrow [H_{2}] = 3 x$

Total moles= $3 - 2 x + x + 3 x = 3 + 2 x$

Concentration of $N H_{3}$ at $t = 10$ ,

$\Rightarrow [N H_{3}] = (- 0.1 \times 10) + 3$
$= - 1 + 3 = 2 a t m$
$∴ 3 - 2 x = 2$
$\Rightarrow 3 - 2 = 2 x$
$\Rightarrow 2 x = 1$
$\Rightarrow x = 0.5$

$∴$ Total pressure= $3 + 2 x = 3 + 2 (0.5)$
$= 3 + 1$
$= 4 a t m$ .

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