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Characteristics of Chemical Equilibrium

Find moles of...

Question

Find moles of $N_{2} O_{4}$ and $N O_{2}$ at equilibrium are $1$ and $2$ respectively total pressure at equilibrium is $9 a t m$ . Find $K_{P}$ for the reaction $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ .

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Solution

$N_{2} O_{4} (g) ⇌ 2 {N O}_{2} (g)$
$1$ $2$
total pressure (P) = 9 atm
$K_{p} = \frac{{(P_{{N O}_{2}})}^{2}}{P_{N_{2}} O_{4}} \to (1)$
$P_{{N O}_{2}} = Y_{{N O}_{2}} P_{t o t a l}$ (from Dalton's law)
where, $Y_{{N O}_{2}} =$ mole fraction of ${N O}_{2}$
$∴ P_{{N O}_{2}} = (\frac{2}{1 + 2}) \times 9 = \frac{2}{3} \times 9 = 6 a t m \to (2)$
and $P_{N_{2} O_{4}} = \frac{1}{3} \times 9 = 3 a t m \to (3)$
from (1), (2) and (3) we have
$K_{p} = \frac{6^{2}}{3} = \frac{6 \times 6}{3} = 12$

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Similar questions

36.6 g N_{2} O_{4} (g)

is introduced into a

1.0 - l i t r e

27^{\circ} C

. The following equilibrium reaction occurs:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{p} = 0.1642 a t m

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(a) Calculate

K_{c}

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(b) What are the number of moles of

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(c) What is the total gas pressure in the flask at equilibrium?
(d) What is the percent dissociation of

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Q. When the reaction,

2 N O_{2} (g) ⇌ N_{2} O_{4} (g)

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0.4

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Q. For the reaction equilibrium

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4.5

What would be the average molar mass (in g/mol) of an equilibrium mixture of

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