The density of an equilibrium mixture of N 2 O 4 and NO 2 at 101 . 32 KP a is 3 . 62 gdm - 3 at 288 K and 1 . 84 gdm - 3 at 348 K . What is the heat of the reaction for N 2 O 4 ⇌ 2 NO 2 ( g ) .

Equilibrium - It is the state at which the concentration of reactant and products remain same. M average = ρRT P At 288 K , M average = 3 . 62 × 0 . 0821 × 288 1 = 85 . 6 Let Mole fraction of N 2 O 4 = x Mole Fraction of NO 2 = 1 - x M average = 92 x + 46 1 - x 1 85 . 6 = 92 x + 46 1 - x x = 0 . 85 Mole fraction of N 2 O 4 = 0 . 85 Mole fraction of NO 2 = 0 . 15 Partial Pressure = Mole Fraction × Total Pressure Total Pressure = 1 atm so, Partial Pressure = Mole Fraction K p 1 = P NO 2 2 P N 2 O 4 = 0 . 15 2 0 . 85 = 0 . 0228 Similarly at 348 K M average = 1 . 84 × 0 . 0821 × 348 1 = 52 . 57 M average = 92 x + 46 1 - x 1 = 52 . 57 x = 0 . 14 Mole fraction of N 2 O 4 = 0 . 14 Mole fraction of NO 2 = 0 . 86 K P 2 = 0 . 86 2 0 . 14 = 5 . 282 log K P 2 K p 1 = ΔH ° 2 . 303 R 1 T 1 - 1 T 2 log 5 . 282 0 . 0228 = △ H 2 × 2 . 303 1 288 - 1 348 △ H = 181956 cal = 18 . 196 Kcal = 76 . 106 Kj

The equilibrium constant for the following reaction at 1395 K . 2 H 2 O ⇌ 2 H 2 + O 2 K 1 = 2 . 1 × 10 - 13 2 CO 2 ⇌ 2 CO + O 2 K 2 = 1 . 4 × 10 - 12 Calculate the value of K for the reaction : H 2 + CO 2 ⇌ CO + H 2 O

Equilibrium Constant - It is the ratio of concentration of products and reactants each raise to its stoichiometric constant. 2 H 2 O ⇋ 2 H 2 g + O 2 K 1 = 2 . 1 × 10 - 13 Reverse this reaction 2 H 2 g + O 2 g ⇌ 2 H 2 O K ' = 1 K 1 . . . . . . . 1 2 CO 2 g ⇋ 2 CO + O 2 K 2 = 1 . 4 × 10 - 12 . . . . . . 2 Add equation 1 and 2 2 H 2 + 2 CO 2 ⇌ 2 CO + 2 H 2 O K 3 = 1 K 1 × K 2 . . . . . 3 Divide equation 3 by 2 H 2 + CO 2 ⇋ CO + H 2 O K 3 = K 2 K 1 K 3 = 1 . 4 × 10 - 12 2 . 1 × 10 - 13 = 2 . 58

EASY

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IMPORTANT

Earn 100

The degree of dissociation of $HI$ at a particular temperature is $0.8 .$ Find the volume of $1.5 M$ sodium thiosulphate solution required to react completely with the iodine present at equilibrium in acidic conditions, when $0.135$ mol each of $H_{2}$ and $I_{2}$ are heated at $440 K$ in a closed vessel of capacity $2.0 L .$

Important Questions on Equilibrium

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 5

The equilibrium constant for the reaction

CO (g) + H_{2} O (g) ⇌ {CO}_{2} (g) + H_{2} (g)

7.3

450 ° C & 1 atm

pressure. The initially concentration of water gas [CO

& H_{2}

in equimolar ratio]

&

steam are

2

moles

& 5

moles respectively. Find the number of moles of

CO, H_{2}, {CO}_{2} & H_{2} O

(vapour) at equilibrium.

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 6

At $1200 ° C$ , the following equilibrium is established between chlorine atoms & molecule.

${Cl}_{2} (g) ⇌ 2 Cl (g)$

The composition of equilibrium mixture may be determined by measuring the rate of effusion of the mixture through a pin hold. It is found that at $1200 ° C$ and $1$ atm pressure the mixture effuses $1.16$ times as fast as krypton effuses under the same condition. Calculate the equilibrium constant $K_{c}$ .

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 7

Two solids $X$ and $Y$ dissociate into gaseous products at a certain temperature as follows :
$X (s) ⇌ A (g) + C (g)$ , and $Y (s) ⇌ B (g) + C (g)$ . At a given temperature, pressure over excess solid $X$ is $40 mm$ and total pressure over solid $Y$ is $60 mm$ . Calculate :

(a) the values of $K_{p}$ for two reactions (in $mm$ )

(b) the ratio of moles of $A$ and $B$ in the vapour state over a mixture of $X$ and $Y$ .

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 8

{SO}_{3}

decomposes at a temperature of

1000 K

and at a total pressure of

1.642 atm

. At equilibrium, the density of mixture is found to be

1.28 g L^{- 1}

in a vessel of

90

litres. Find the degree of dissociation of

{SO}_{3}

for

{SO}_{3} ⇌ {SO}_{2} + \frac{1}{2 O_{2}}

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 9

The density of an equilibrium mixture of

N_{2} O_{4}

and

{NO}_{2}

101.32 {KP}_{a}

3.62 {gdm}^{- 3}

288 K

and

1.84 {gdm}^{- 3}

348 K

. What is the heat of the reaction for

N_{2} O_{4} ⇌ 2 {NO}_{2} (g)

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 10

The equilibrium constant for the following reaction at $1395 K$ .

$2 H_{2} O ⇌ 2 H_{2} + O_{2} K_{1} = 2.1 \times 10^{- 13}$

$\begin{array}{l} 2 {CO}_{2} ⇌ 2 CO + O_{2} & K_{2} = 1.4 \times 10^{- 12} \end{array}$

Calculate the value of $K$ for the reaction : $H_{2} + {CO}_{2} ⇌ CO + H_{2} O$

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 11

A saturated solution of iodine in water contains

0.33 {gI}_{2} L^{- 1}

. More than this can dissolve in a

KI

solution because of the equilibrium :

I_{2} (aq) + I^{-} (aq) ⇌ I_{3}^{-} (aq)

. A

0.10 MKI

solution

(0.10 {MI}^{-})

actually dissolves

12.5 g

of iodine

/ L

, most of which is converted to

I_{3}^{-}

. Assuming that the concentration of

I_{2}

in all saturated solutions is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated of

I_{2}

in the

KI

solution?

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 12

A mixture of

N_{2}

H_{2}

are in equilibrium at

600 K

at a total pressure of

80 atm

. If the initial ratio of

N_{2}

and

H_{2}

are

3 : 1

and at equilibrium

{NH}_{3}

10 %

by volume, calculate

K_{p}

of reaction at given temperature.

Important Questions on Equilibrium

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