For the given reaction at equilibrium: AgNO 3 ( s ) ⇌ Ag ( s ) + NO 2 ( g ) + 1 2 O 2 ( g ) If total pressure at equilibrium is P , then calculate K p for the given reaction.

Given reaction AgNO 3 ( s ) ⇌ Ag ( s ) + NO 2 ( g ) + 1 2 O 2 ( g ) At t = 0 1 0 0 0 At t = eq 1 - P ' P ' P ' P ' 2 But partial pressure of solids is considered as unity. Given total pressure at equilibrium is P and pressure is due to only gases here which are NO 2 & O 2 P NO 2 + P O 2 = P So, P ' + P ' 2 = P P ' = 2 P 3 So, P NO 2 = P ' = 2 P 3 P O 2 = P ' 2 = P 3 Now, K p = P NO 2 . P O 2 1 2 K p = 2 P 3 × P 3 1 2 K p = 2 P 3 2 3 3

From the following data i. H 2 ( g ) + CO 2 ( g ) ⇌ H 2 O ( g ) + CO ( g ) ; K 2000 K = 4 . 40 ii. 2 H 2 O ( g ) ⇌ 2 H 2 ( g ) + O 2 ( g ) ; K 2000 K 1 = 5 . 31 × 10 - 10 iii. 2 CO ( g ) + O 2 ( g ) ⇌ 2 CO 2 ( g ) ; K 1000 K = 2 . 24 × 10 22 Show whether reaction (iii) is exothermic or endothermic.

Let us consider reactions (i) and (ii) Multiplying reaction (i) by 2 , we get 2 H 2 ( g ) + 2 CO 2 ( g ) ⇌ 2 H 2 O ( g ) + 2 CO ( g ) . . . i v K 2000 K Il = K 2000 K 2 = ( 4 . 40 ) 2 Adding (iv) and (ii), we have 2 CO 2 ( g ) ⇌ 2 CO + O 2 K 2000 K III = K 2000 K II × K 2000 K I = ( 4 . 40 ) 2 × 5 . 31 × 10 - 10 Therefore, by reversing the reaction, we get reaction but at 2000 K 2 CO ( g ) + O 2 ( g ) ⇌ 2 CO 2 ( g ) ; for which K 2000 K IV = 1 K III 2000 K = 1 4 . 40 2 × 5 . 31 × 10 - 10 = 9 . 72 × 10 7 From reactions (iii) and (v), we see that as the temperature increases, the equilibrium constant decreases 9 . 72 × 10 7 < 2 . 24 × 10 22 ). Reaction (iii) is thus exothermic because Δ H will be negative.

The exothermic formation of ClF 3 is represented by the following equation: Cl 2 g + 3 F 2 g ⇌ 2 ClF 3 g ; ΔH = - 329 kJ Which of the following will increase the quantity of ClF 3 in the equilibrium mixture of Cl 2 , F 2 and ClF 3 ?

Increasing the volume of the container.

EASY

JEE Main/Advance

IMPORTANT

Earn 100

Write the expressions for equilibrium constant $K_{C}$ and $K_{p}$ . Classify in Homogeneous and Heterogeneous equilibrium:

${NH}_{4} HS (s) ⇌ {NH}_{3} (g) + H_{2} S (g)$

Important Questions on Equilibrium

EASY

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 90

Write the expressions for equilibrium constant $K_{C}$ and $K_{p}$ . Classify in Homogeneous and Heterogeneous equilibrium:

${CH}_{3} COOH (ℓ) + C_{2} H_{5} OH (ℓ) ⇌ {CH}_{3} {COOC}_{2} H_{5} (ℓ) + H_{2} O (ℓ)$

EASY

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 91

Write the expressions for equilibrium constant $K_{C}$ and $K_{p}$ . Classify in Homogeneous and Heterogeneous equilibrium:

${MgCO}_{3} (s) ⇌ MgO (s) + {CO}_{2} (g)$

MEDIUM

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 94

Write the expressions for equilibrium constant $K_{C}$ and $K_{p}$ classify in homogeneous and heterogeneous equilibrium:

${NH}_{4} {NO}_{2} (s) ⇌ N_{2} (g) + 2 H_{2} O (l)$

HARD

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 95

For the given reaction at equilibrium:

${AgNO}_{3} (s) ⇌ Ag (s) + {NO}_{2} (g) + \frac{1}{2} O_{2} (g)$

If total pressure at equilibrium is $P$ , then calculate $K_{p}$ for the given reaction.

HARD

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 96

N_{2} O_{4}

25 %

dissociated at

37 ° C

and one-atmosphere pressure. Calculate

(i)

K_{p}

and

(ii)

the percentage dissociation at

0.1

atmosphere and

37 ° C

HARD

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 97

At temperature

T,

the compound

{AB}_{2} (g)

dissociates according to the reaction;

2 {AB}_{2} (g) ⇌ 2 AB (g) + B_{2} (g)

.
With a degree of dissociation

x,

which is small compared with unity. Deduce the expression for

x

in terms of the equilibrium constant,

K_{p}

and the total pressure,

P

MEDIUM

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 99

From the following data
i.

H_{2} (g) + {CO}_{2} (g) ⇌ H_{2} O (g) + CO (g); K_{2000 K} = 4.40

ii.

2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g); K_{2000 K}^{1} = 5.31 \times 10^{- 10}

iii.

2 CO (g) + O_{2} (g) ⇌ 2 {CO}_{2} (g); K_{1000 K} = 2.24 \times 10^{22}

Show whether reaction (iii) is exothermic or endothermic.

HARD

JEE Main/Advance

IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-1>Q 104

When $NO$ and ${NO}_{2}$ are mixed, the following equilibria are readily obtained;

$2 {NO}_{2} ⇌ N_{2} O_{4} K_{P} = 6.8 {atm}^{- 1}$

and $NO + {NO}_{2} ⇌ N_{2} O_{3}$

In an experiment when $NO$ and ${NO}_{2}$ are mixed in the ratio of $1 : 2$ , the final total pressure was $5.05 atm$ and the partial pressure of $N_{2} O_{4}$ was $1.7 atm$ . Calculate :
(a) the equilibrium partial pressure of $NO$ .
(b) $K_{P}$ for $NO + {NO}_{2} ⇌ N_{2} O_{3}$ .

Write the expressions for equilibrium constant KC and Kp. Classify in Homogeneous and Heterogeneous equilibrium: NH4HS(s)⇌NH3(g)+H2S(g)

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

Write the expressions for equilibrium constant $K_{C}$ and $K_{p}$ . Classify in Homogeneous and Heterogeneous equilibrium:

${NH}_{4} HS (s) ⇌ {NH}_{3} (g) + H_{2} S (g)$