A ⇌ B . In this reaction, k f is 2 × 10 - 3 and k b is 5 × 10 - 4 . Determine the value of K c .

The ratio of rate constant of forward direction and backward direction is known as equilibrium constant: K C = k f k b = 2 × 10 - 3 5 × 10 - 4 = 20 5 = 4

2 moles of PCl 5 when heated in a closed vessel of 2 litre capacity at equilibrium 40 % of PCl 5 dissociated in PCl 3 and Cl 2 . What is the value of the equilibrium constant?

For the given reaction, according to the question: PCl 5 ⇌ PCl 3 + Cl 2 t = 0 2 t = t equilibrium 2 - 0 . 8 0 . 8 0 . 8 So, PCl 5 = 1 . 2 2 = 0 . 6 ; PCl 3 = 0 . 8 2 = 0 . 4 Cl 2 = 0 . 8 2 = 0 . 4 The equilibrium constant: K C = PCl 3 Cl 2 PCl 5 = 0 . 4 × 0 . 4 0 . 6 = 1 . 6 0 . 6 = 0 . 267

MEDIUM

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IMPORTANT

Earn 100

$4$ moles of ${PCl}_{5}$ are heated at constant temperature in closed container. If degree of dissociation for ${PCl}_{5}$ is $0.5$ calculate total number of moles at equilibrium.

Important Questions on Chemical Equilibrium

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IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 44

For the reaction

3 A (g) + B (g) ⇌ 2 C (g)

at a given temperature,

K_{c} = 9.0

. What must be the volume of the flask, if a mixture of

2.0 mol

each of

A, B

and

C

exist in equilibrium?

MEDIUM

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IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 45

4.5

moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium,

3

moles of

HI

were found. Determine the equilibrium constant for

H_{2} (g) + I_{2} (g) ⇌ 2 Hl (g)

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IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 46

4

moles of

A

are mixed with

4

moles of

B

, when

2

moles of

C

are formed at equilibrium, according to the reaction,

A + B ⇌ C + D

. Determine equilibrium constant.

MEDIUM

KVPY Aptitude Test - Stream SA

IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 47

A ⇌ B

. In this reaction,

k_{f}

2 \times 10^{- 3}

and

k_{b}

5 \times 10^{- 4}

. Determine the value of

K_{c}

EASY

KVPY Aptitude Test - Stream SA

IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 48

The equilibrium

N_{2} (g) + O_{2} (g) ⇌ 2 NO (g)

established in a reaction vessel of

2.5 L

capacity. The amounts of

N_{2}

and

O_{2}

taken at the start were respectively

2

moles and

4

moles. Half a mole of nitrogen has been used up at equilibrium. What is the molar concentration of nitric oxide?

HARD

KVPY Aptitude Test - Stream SA

IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 49

2

moles of

{PCl}_{5}

when heated in a closed vessel of

2

litre capacity at equilibrium

40 %

{PCl}_{5}

dissociated in

{PCl}_{3}

and

{Cl}_{2}

. What is the value of the equilibrium constant?

HARD

KVPY Aptitude Test - Stream SA

IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>EXERCISE>Q 50

K_{c} = 9

for the reaction,

A + B ⇌ C + D

. If

A

and

B

are taken in equal amounts, then what is the amount of

C

in equilibrium?

HARD

KVPY Aptitude Test - Stream SA

IMPORTANT

Practice Book for KVPY Aptitude Test - Stream SA Chemistry>Chapter 7 - Chemical Equilibrium>KVPY PROBLEMS (PREVIOUS YEARS)>Q 1

When

4

moles of

N_{2}

gas react with

16

moles of

H_{2}

gas in

10

litre vessel,

4

moles of ammonia gas is produced in the equilibrium mixture. The equilibrium constant

K_{c}

for this reaction in

{mol}^{- 2} {lit}^{2}

is:

4 moles of PCl5 are heated at constant temperature in closed container. If degree of dissociation for PCl5 is 0.5 calculate total number of moles at equilibrium.

Important Questions on Chemical Equilibrium

Learn and Prepare for any exam you want !

$4$ moles of ${PCl}_{5}$ are heated at constant temperature in closed container. If degree of dissociation for ${PCl}_{5}$ is $0.5$ calculate total number of moles at equilibrium.