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Standard XII

Chemistry

Derivation of Kp and Kc

In the reacti...

Question

In the reaction $N_{2} O_{4} ⇋ 2 N O_{2}$ , the degree of dissociation of $N_{2} O_{4}$ was found to be 0.4 when the reaction is conducted in a 2 liter vessel. The equilibrium constant $K_{c}$ of the reaction is :

0.53

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1.06

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0.265

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Solution

The correct option is A 0.53
Assume initially 1 mole of $N_{2} O_{4}$ is present.
The following table lists the number of moles of various species.
$N_{2} O_{4}$
$N O_{2}$
Initial
1
0
Change
-0.4
0.8
Equilibrium
0.6
0.8

The volume of the vessel is 2L.
Thus, the equilibrium concentrations of $N_{2} O_{4}$ and $N O_{2}$ are 0.3M and 0.4M respectively.
The expression for the equilibrium constant becomes $K_{c} = \frac{[N O_{2}]^{2}}{[N_{2} O_{4}]} = \frac{(0.4)^{2}}{0.3} = 0.53$ .

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Similar questions

Q. In the reaction

N_{2} O_{4} ⇋ 2 N O_{2}

the degree of dissociation of

N_{2} O_{4}

was found to be 0.4 when the reaction is conducted in a 2 litre vessel. The equilibrium constant

K_{c}

of the reaction is:

Q. Gaseous

N_{2} O_{4}

dissociates into gaseous

N O_{2}

according to the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

at 300 K and 1 atm pressure, the degree of dissociation of

N_{2} O_{4}

is 0.2. If one mole of

N_{2} O_{4}

gas is contained in a vessel, then the density of the equilibrium mixture is :

Q. The equilibrium constant (

K_{c}

) of the reaction

2 S O_{2} + O_{2} ⇋ 2 S O_{3}

, when the reaction is conducted in a one litre vessel was found to be

2.5 \times 10^{- 3}

. If the reaction is conducted at the same temperature in a 2 litre vessel, then the value of

K_{c}

is:

13.8 g

N_{2} O_{4}

was placed in a

1 L

reaction vessel at

400 K

and allowed to attain equilibrium

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

The total pressure at equilibrium was found to be

9.15 B a r

. Calculate

K_{c}, K_{p}

and partial pressure at equilibrium.

Q. Consider the following dissociation reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

What is the

K_{e q}

for the reaction at equilibrium, if the concentration of

N_{2} O_{4}

4 \times 10^{- 2}

mole

/

liter and that of

N O_{2}

2 \times 10^{- 2}

mole

/

liter?

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	$N_{2} O_{4}$	$N O_{2}$
Initial	1	0
Change	-0.4	0.8
Equilibrium	0.6	0.8

In the reaction N2O4⇋2NO2, the degree of dissociation of N2O4 was found to be 0.4 when the reaction is conducted in a 2 liter vessel. The equilibrium constant Kc of the reaction is :

In the reaction $N_{2} O_{4} ⇋ 2 N O_{2}$ , the degree of dissociation of $N_{2} O_{4}$ was found to be 0.4 when the reaction is conducted in a 2 liter vessel. The equilibrium constant $K_{c}$ of the reaction is :