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Chemistry Part-I

Equilibrium

The value of K_{c}=4.24 at 800 {~K} for the reaction, {CO}({g}

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

PCl_{5}, PCl_{3}

and

Cl_{2}

are at equilibrium at

500 K

and having concentration

1.59 M

PCl_{3}, 1.59 M Cl_{2}

and

1.41 M PCl_{5}

. Calculate

K_{c}

for the reaction,

PCl_{5} ⇌ PCl_{3} + Cl_{2}

The value of

K_{c} = 4.24

800 K

for the reaction,

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

Calculate equilibrium concentrations of

CO_{2}, H_{2}, CO

and

H_{2} O

800 K

, if only

CO

and

H_{2} O

are present initially at concentrations of

0.10 M

each.

For the equilibrium,

2 NOCl (g) ⇌ 2 NO (g) + Cl_{2} (g)

the value of the equilibrium constant,

K_{c}

3.75 \times 1 0^{- 6}

1069 K

. Calculate the

K_{p}

for the reaction at this temperature?

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Question

Easy

Solving time: 2 mins

The value of $K_{c} = 4.24$ at $800 K$ for the reaction, $CO (g) + H_{2} O (g) ⇌ CO_{2} (g) + H_{2} (g)$

Calculate equilibrium concentrations of $CO_{2}, H_{2}, CO$ and $H_{2} O$ at $800 K$ , if only $CO$ and $H_{2} O$ are present initially at concentrations of $0.10 M$ each.

Views: 5,342 students

Updated on: Sep 24, 2023

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Chemistry Part-I (NCERT)

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The value of

K_{c} = 4.24

800 K

for the reaction,

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

Calculate equilibrium concentrations of

CO_{2}, H_{2}, CO

and

H_{2} O

800 K

, if only

CO

and

H_{2} O

are present initially at concentrations of

0.10 M

each.

6 mins ago

Discuss this question LIVE

6 mins ago

Text solutionVerified

Solution
For the reaction,

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

Initial concentration:

0.1 M 0.1 M 00

Let

x

mole per litre of each of the product be formed.
At equilibrium:

(0.1 - x) M

(0.1 - x) M x M x M

where

x

is the amount of

CO_{2}

and

H_{2}

at equilibrium.

Hence, equilibrium constant can be written as,

K_{c} = x^{2} / (0.1 - x)^{2} = 4.24

x^{2} = 4.24 (0.01 + x^{2} - 0.2 x)

x^{2} = 0.0424 + 4.24 x^{2} - 0.848 x

3.24 x^{2} - 0.848 x + 0.0424 = 0

a = 3.24, b = - 0.848, c = 0.0424

(for quadratic equation

ax^{2} + bx + c = 0

x = \frac{( - b \pm b ^{2} - 4 a c )}{2 a}

x = 0.848 \pm (0.848)^{2} - 4 (3.24) (0.0424)

(3.24 \times 2)

x = (0.848 \pm 0.4118) /6.48

x_{1} = (0.848 - 0.4118) /6.48 = 0.067

x_{2} = (0.848 + 0.4118) /6.48 = 0.194

the value

0.194

should be neglected because it will give concentration of the reactant which is more than initial concentration.

Hence the equilibrium concentrations are,

[CO_{2}] = [H_{2}] = x = 0.067 M

[CO] = [H_{2} O] = 0.1 - 0.067 = 0.033 M

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Practice more questions from Chemistry Part-I (NCERT)

PCl_{5}, PCl_{3}

and

Cl_{2}

are at equilibrium at

500 K

and having concentration

1.59 M

PCl_{3}, 1.59 M Cl_{2}

and

1.41 M PCl_{5}

. Calculate

K_{c}

for the reaction,

PCl_{5} ⇌ PCl_{3} + Cl_{2}

The value of

K_{c} = 4.24

800 K

for the reaction,

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

Calculate equilibrium concentrations of

CO_{2}, H_{2}, CO

and

H_{2} O

800 K

, if only

CO

and

H_{2} O

are present initially at concentrations of

0.10 M

each.

For the equilibrium,

2 NOCl (g) ⇌ 2 NO (g) + Cl_{2} (g)

the value of the equilibrium constant,

K_{c}

3.75 \times 1 0^{- 6}

1069 K

. Calculate the

K_{p}

for the reaction at this temperature?

View all

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Question Text	The value of $K_{c} = 4.24$ at $800 K$ for the reaction, $CO (g) + H_{2} O (g) ⇌ CO_{2} (g) + H_{2} (g)$ Calculate equilibrium concentrations of $CO_{2}, H_{2}, CO$ and $H_{2} O$ at $800 K$ , if only $CO$ and $H_{2} O$ are present initially at concentrations of $0.10 M$ each.
Updated On	Sep 24, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 3
Upvotes	426
Avg. Video Duration	10 min

The value of $K_{c} = 4.24$ at $800 K$ for the reaction, $CO (g) + H_{2} O (g) ⇌ CO_{2} (g) + H_{2} (g)$

Calculate equilibrium concentrations of $CO_{2}, H_{2}, CO$ and $H_{2} O$ at $800 K$ , if only $CO$ and $H_{2} O$ are present initially at concentrations of $0.10 M$ each.

Text solutionVerified

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The value of Kc​=4.24 at 800 K for the reaction, CO(g)+H2​O(g)⇌CO2​( g)+H2​( g) Calculate equilibrium concentrations of CO2​,H2​,CO and H2​O at 800 K, if only CO and H2​O are present initially at concentrations of 0.10M each.

Text solutionVerified

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The value of $K_{c} = 4.24$ at $800 K$ for the reaction, $CO (g) + H_{2} O (g) ⇌ CO_{2} (g) + H_{2} (g)$

Calculate equilibrium concentrations of $CO_{2}, H_{2}, CO$ and $H_{2} O$ at $800 K$ , if only $CO$ and $H_{2} O$ are present initially at concentrations of $0.10 M$ each.