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Characteristics of Equilibrium Constant

The value of ...

Question

The value of $K_{c}$ for the reaction
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)$
is $0.50$ at $400^{o} C$ . Find the value of $K_{p}$ at $400^{o} C$ when concentrations are expressed in $m o l$ ${l i t r e}^{- 1}$ and pressure in atmosphere.

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Solution

Applying the relationship
$K_{p} = K_{c} {(R T)}^{Δ n}$
$K_{c} = 0.50$ , $R = 0.082 l i t r e - a t m {d e g C}^{- 1} {m o l}^{- 1}$
$T = (400 + 273) K = 673 K$ , $Δ n = (2 - (1 + 3)) = - 2$
$K_{p} = 0.50 \times {(0.082 \times 673)}^{- 2} = 0.50 \times {(55.185)}^{- 2} = 1.64 \times 10^{- 4}$

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