Nitrogen dioxide forms dinitrogen tetroxide according to the equation 2 NO 2 g ⇌ N 2 O 4 g When 0 . 1 mole of NO 2 is added to a 1 litre flask at 25 ∘ C , the concentration changes so that at equilibrium NO 2 = 0 . 016 M and N 2 O 4 = 0 . 042 M a) What is the value of the reaction Quotient before any reaction occurs.

2 NO 2 g ⇌ N 2 O 4 g (The combination of nitrogen dioxide dimer ) Before any product is formed, NO 2 = 0 . 10 mol 1 . 0 L = 0 . 10 M , and N 2 O 4 = 0 M Thus, Q c = N 2 O 4 NO 2 2 = 0 0 . 10 2 = 0

Nitrogen dioxide forms dinitrogen tetroxide according to the equation 2 NO 2 g ⇌ N 2 O 4 g When 0 . 1 mole of NO 2 is added to a 1 litre flask at 25 ∘ C , the concentration changes so that at equilibrium NO 2 = 0 . 016 M and N 2 O 4 = 0 . 042 M a) What is the value of the reaction Quotient before any reaction occurs.

2 NO 2 g ⇌ N 2 O 4 g (The combination of nitrogen dioxide dimer ) Before any product is formed, NO 2 = 0 . 10 mol 1 . 0 L = 0 . 10 M , and N 2 O 4 = 0 M Thus, Q c = N 2 O 4 NO 2 2 = 0 0 . 10 2 = 0

Nitrogen dioxide forms dinitrogen tetroxide according to the equation 2 NO 2 g ⇌ N 2 O 4 g When 0 . 1 mole of NO 2 is added to a 1 litre flask at 25 ∘ C , the concentration changes so that at equilibrium NO 2 = 0 . 016 M and N 2 O 4 = 0 . 042 M b) What is the value of equilibrium constant for the reaction.

2 NO 2 g ⇌ N 2 O 4 g At equilibrium, the value of equilibrium constant is equal to the value of the reaction quotient. At equilibrium: K c = Q c = N 2 O 4 NO 2 = 0 . 042 0 . 016 2 = 1 . 6 × 10 2 The equilibrium constant is 1 . 6 × 10 2

Under certain conditions, the equilibrium constant for the decomposition of PCl 5 g into PCl 3 g and Cl 2 g is 0 . 0211 mol L - 1 . What are the equilibrium concentrations of PCl 5 , PCl 3 and Cl 2 , if the initial concentration of PCl 5 was 1 . 00 M ?

PCl 5 g ⏟ 1 - x ⇌ PCl 3 g ⏟ x + Cl 2 g ⏟ x The equilibrium constant for K c for the reaction is 0 . 0211 K c = PCl 3 Cl 2 PCl 5 = 0 . 0211 = x x 1 - x = 0 . 0211 = 0 . 0211 1 - x = x 2 x 2 + 0 . 0211 x - 0 . 0211 = 0 ∴ ax 2 + bx + c = 0 x = - 0 . 0211 ± 0 . 0211 2 - 4 1 - 0 . 0211 2 1 x = - b ± b 2 - 4 ac 2 a = - 0 . 0211 ± 4 . 45 × 10 - 4 + 8 . 44 × 10 - 2 2 = - 0 . 0211 ± 0 . 291 2 x = - 0 . 0211 + 0 . 291 2 = 0 . 135 or x = - 0 . 0211 - 0 . 291 2 = - 0 . 156 so , PCl 5 = 1 . 00 - 0 . 135 = 0 . 87 M PCl 3 = x = 0 . 135 M Cl 2 = x = 0 . 135 M

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11th Telangana Board

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Earn 100

Nitrogen dioxide forms dinitrogen tetroxide according to the equation $2 {NO}_{2} (g) ⇌ N_{2} O_{4} (g)$ When $0.1 mole of {NO}_{2}$ is added to a $1$ litre flask at $25^{\circ} C$ , the concentration changes so that at equilibrium $[{NO}_{2}] = 0.016 M and [N_{2} O_{4}] = 0.042 M$

a) What is the value of the reaction Quotient before any reaction occurs.

Important Questions on Chemical Equilibrium and Acids - Bases

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 2

Nitrogen dioxide forms dinitrogen tetroxide according to the equation $2 {NO}_{2} (g) ⇌ N_{2} O_{4} (g)$ When $0.1 mole of {NO}_{2}$ is added to a $1$ litre flask at $25^{\circ} C$ , the concentration changes so that at equilibrium $[{NO}_{2}] = 0.016 M and [N_{2} O_{4}] = 0.042 M$

b) What is the value of equilibrium constant for the reaction.

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 3

The equilibrium constant for the reaction:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g)

At equilibrium

[H_{2}] = 0.25 mol L^{- 1}

and

[N H_{3}] = 0.06 mol L^{- 1}

. Calculate the equilibrium concentration of

N_{2}

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 4

At certain temperature,

K_{c}

for the reaction.

{SO}_{2} (g) + {NO}_{2} (g) ⇌ {SO}_{3} (g) + NO (g)

16

. If initially one mole each of all the four gases are taken in one litre vessel. What are the equilibrium concentrations

NO and {NO}_{2}

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 5

Under certain conditions, the equilibrium constant for the decomposition of

{PCl}_{5} (g)

into

{PCl}_{3} (g)

and

{Cl}_{2} (g)

0.0211 mol L^{- 1}

. What are the equilibrium concentrations of

{PCl}_{5}, {PCl}_{3} and {Cl}_{2}

, if the initial concentration of

{PCl}_{5} was 1.00 M

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 6

For the reaction

A + B ⇌ 3 C at 25^{\circ} C

, a

3

litre vessel contains

1, 2, 4 moles of A, B and C

respectively predict the direction of reaction if

K_{c}

for the reaction is

10

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 6

For the reaction

A + B ⇌ 3 C at 25^{\circ} C

, a

3

litre vessel contains

1, 2, 4 moles of A, B and C

respectively predict the direction of reaction if

K_{c}

for the reaction is

15

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 6

For the reaction

A + B ⇌ 3 C at 25^{\circ} C

, a

3

litre vessel contains

1, 2, 4 moles of A, B and C

respectively predict the direction of reaction if

K_{c}

for the reaction is

10.66

HARD

11th Telangana Board

IMPORTANT

Intermediate First Year Chemistry>Chapter 7 - Chemical Equilibrium and Acids - Bases>QUESTIONS>Q 7

A mixture of $H_{2}, N_{2} and {NH}_{3}$ with molar concentrations $5 \times 10^{- 3} mol L^{- 1}$ , $4 \times 10^{- 3} mol L^{- 1}$ and $2 \times 10^{- 3} mol L^{- 1}$ , respectively was prepared and heated to $500 K$ .The value of $K_{c}$ for the reaction: $3 H_{2} (g) + N_{2} (g) ⇌ 2 {NH}_{3} (g)$ at this temperature is $60$ . Predicts whether ammonia tends to form or decompose at this stage of concentration.

Nitrogen dioxide forms dinitrogen tetroxide according to the equation 2NO2g⇌N2O4g When 0.1 mole of NO2 is added to a 1 litre flask at 25∘C, the concentration changes so that at equilibrium NO2=0.016M and N2O4=0.042M a) What is the value of the reaction Quotient before any reaction occurs.

Important Questions on Chemical Equilibrium and Acids - Bases

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