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Chemistry Part-I

Equilibrium

Equilibrium constant, K_{c} for the reaction, N_{2(g)} + 3H_{2

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

A sample of pure

PCl_{5}

was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of

PCl_{5}

was found to be

0.5 \times 10^{- 1} m o l L^{- 1}

. If value of

K_{c}

8.3 \times 10^{- 3}

, what are the concentrations of

PCl_{3}

and

Cl_{2}

at equilibrium?

PCl_{5} (g) ⇌ PCl_{3} (g) + Cl_{2} (g)

Equilibrium constant,

K_{c}

for the reaction,

N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}

; at

500 K

0.061 l i t r e^{2} m o l e^{- 2}

. At a particular time, the analysis shows that composition of the reaction mixture is

3.00 m o l l i t r e^{- 1}

N^{2}

2.00 m o l l i t r e^{- 1}

H_{2}

, and

0.500 m o l l i t r e^{- 1}

N H_{3}

. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

Bromine monochloride,

B r Cl

, decomposes into broe and chlorine and reaches equilibrium as

2 B r C l_{(g)} ⇌ B r_{2 (g)} + C l_{2 (g)}

; for which

K_{c} = 32

500 K

B r Cl

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Question

Medium

Solving time: 4 mins

Equilibrium constant, $K_{c}$ for the reaction, $N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}$ ; at $500 K$ is $0.061 l i t r e^{2} m o l e^{- 2}$ . At a particular time, the analysis shows that composition of the reaction mixture is $3.00 m o l l i t r e^{- 1}$ of $N^{2}$ , $2.00 m o l l i t r e^{- 1}$ of $H_{2}$ , and $0.500 m o l l i t r e^{- 1}$ of $N H_{3}$ . Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

Name: Video solution 1: [Solved] Equilibrium constant, Kc for the reaction, N2(g)+3H2(g)⇌ 2NH3(g); at 500 K is 0.061 litre2 mole−2. At a particular time, the analysis shows that composition of the reaction mixture is 3.00 mol litre−1 of N2, 2.00 mol litre−1 of H2, and 0.500 mol litre−1 of NH3. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium? - Chemistry Part-I
Uploaded: 2022-02-05T20:45:40.000Z
Duration: 14 min

Views: 6,229 students

Updated on: Feb 5, 2022

Book:

Chemistry Part-I (NCERT)

Found 4 tutors discussing this question

Elijah Discussed

Equilibrium constant,

K_{c}

for the reaction,

N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}

; at

500 K

0.061 l i t r e^{2} m o l e^{- 2}

. At a particular time, the analysis shows that composition of the reaction mixture is

3.00 m o l l i t r e^{- 1}

N^{2}

2.00 m o l l i t r e^{- 1}

H_{2}

, and

0.500 m o l l i t r e^{- 1}

N H_{3}

. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

10 mins ago

Discuss this question LIVE

10 mins ago

Text solutionVerified

Q_{c} = \frac{[ N H _{3} ] ^{2}}{[ N _{2} ] [ H _{2} ] ^{3}}

Q = \frac{( 0.50 ) ^{2}}{( 3.0 ) ( 2.0 ) ^{3}} = 0.0104

The value of the reaction quotient is not equal to the value of the equilibrium constant.
Hence, the reaction is not at equilibrium.
The value of the reaction quotient is less than the value of the equilibrium constant.
Hence, the reaction will proceed to form more products, i.e., in the forward direction.

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Practice more questions from Chemistry Part-I (NCERT)

A sample of pure

PCl_{5}

was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of

PCl_{5}

was found to be

0.5 \times 10^{- 1} m o l L^{- 1}

. If value of

K_{c}

8.3 \times 10^{- 3}

, what are the concentrations of

PCl_{3}

and

Cl_{2}

at equilibrium?

PCl_{5} (g) ⇌ PCl_{3} (g) + Cl_{2} (g)

Equilibrium constant,

K_{c}

for the reaction,

N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}

; at

500 K

0.061 l i t r e^{2} m o l e^{- 2}

. At a particular time, the analysis shows that composition of the reaction mixture is

3.00 m o l l i t r e^{- 1}

N^{2}

2.00 m o l l i t r e^{- 1}

H_{2}

, and

0.500 m o l l i t r e^{- 1}

N H_{3}

. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

Bromine monochloride,

B r Cl

, decomposes into broe and chlorine and reaches equilibrium as

2 B r C l_{(g)} ⇌ B r_{2 (g)} + C l_{2 (g)}

; for which

K_{c} = 32

500 K

B r Cl

View all

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Question Text	Equilibrium constant, $K_{c}$ for the reaction, $N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}$ ; at $500 K$ is $0.061 l i t r e^{2} m o l e^{- 2}$ . At a particular time, the analysis shows that composition of the reaction mixture is $3.00 m o l l i t r e^{- 1}$ of $N^{2}$ , $2.00 m o l l i t r e^{- 1}$ of $H_{2}$ , and $0.500 m o l l i t r e^{- 1}$ of $N H_{3}$ . Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?
Updated On	Feb 5, 2022
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	165
Avg. Video Duration	14 min

Text solutionVerified

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Text solutionVerified

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