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Characteristics of Equilibrium Constant

When 36.8g ...

Question

When 36.8g $N_{2} O_{4}$ is introduced into a 1 litre flask at 300 K. The following reaction occurs:
$N_{2} O_{4} (g) ⇌ 2 {N O}_{2} (g)$ , $K_{P} = 0.1642$ atm.
Calculate the $K_{C}$ of the equilibrium reaction.

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Solution

${N_{2} O_{4}}_{(g)} ⇌ {2 N O_{2}}_{(g)}$ ; $K_{p} = 0.1642 a t m$
$K_{P} = K_{C} (R T)^{Δ n}$ $Δ n = 2 - 1 = 1$ , $R = 0.0820 L$ $m o l^{- 1} k^{- 1}, T = 300 K$
$\Rightarrow 0.1642 = K_{C} (0.082 \times 300)^{1}$
$\Rightarrow K_{C} = \frac{0.1642}{24.6}$
$= 0.00667 = 6.67 \times 10^{- 3} m o l d m^{- 3}$

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