[Solved] Find out the value of Kc for each of the following equilibria from the value of Kp:(a) 2NOCl(g)⇌2NO(g)+Cl2(g) ; Kp=1.8×10−2atm at 500 K(b) CaCO3(s)⇌CaO(s)+CO2(g) ; Kp=167 atm at 1073 K - Chemistry Part-I

For reaction (a), change in number of moles (Δn)= Number of moles of products − Number of moles of reactants ⇒Δn=3−2=1T=500 K (Given)We know that, Kp=Kc(RT)Δn∴Kc=(RT)△nKp,R=0.0821 litre atm K−1 mol−1⇒Kc=[(0.0821)(500)]11.8×10−2=4.38×10−4For reaction (b), Δn=2−1=1T=1073 K (Given)∴Kc=[(0.0821)(1073)]1167=1.90

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Chemistry Part-I

Equilibrium

Find out the value of K_{c} for each of the following equilibr

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

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (a)

O H^{-}

(b)

F^{-}

(c)

H^{+}

(d)

BCl_{3}

Find out the value of

K_{c}

for each of the following equilibria from the value of

K_{p}

(a)

2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m

500 K

(b)

C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m

1073 K

The degree of ionization of a

0.1 M

bromoacetic acid solution is

0.132

. Calculate the

p H

of the solution and the

p K_{a}

of bromoacetic acid.

View all question

Question

Medium

Solving time: 4 mins

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$ :

(a) $2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m$ at $500 K$

(b) $C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m$ at $1073 K$

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Updated on: Feb 26, 2023

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Chemistry Part-I (NCERT)

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Find out the value of

K_{c}

for each of the following equilibria from the value of

K_{p}

(a)

2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m

500 K

(b)

C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m

1073 K

12 mins ago

Discuss this question LIVE

12 mins ago

Text solutionVerified

For reaction (a), change in number of moles

(Δ n) =

Number of moles of products

-

Number of moles of reactants

\Rightarrow Δ n = 3 - 2 = 1

T = 500 K

(Given)

We know that,

K_{p} = K_{c} (RT)^{Δ n}

∴ K_{c} = \frac{K _{p}}{( RT ) ^{△ n}}

R = 0.0821 l i t re a t m K^{- 1} m o l^{- 1}

\Rightarrow K_{c} = \frac{1.8 \times 1 0 ^{- 2}}{[( 0.0821 ) ( 500 ) ] ^{1}} = 4.38 \times 1 0^{- 4}

For reaction (b),

Δ n = 2 - 1 = 1

T = 1073 K

(Given)

∴ K_{c} = \frac{167}{[( 0.0821 ) ( 1073 ) ] ^{1}} = 1.90

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Practice more questions from Chemistry Part-I (NCERT)

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (a)

O H^{-}

(b)

F^{-}

(c)

H^{+}

(d)

BCl_{3}

Find out the value of

K_{c}

for each of the following equilibria from the value of

K_{p}

(a)

2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m

500 K

(b)

C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m

1073 K

The degree of ionization of a

0.1 M

bromoacetic acid solution is

0.132

. Calculate the

p H

of the solution and the

p K_{a}

of bromoacetic acid.

View all

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Question Text	Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$ : (a) $2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m$ at $500 K$ (b) $C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m$ at $1073 K$
Updated On	Feb 26, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 6
Upvotes	762
Avg. Video Duration	6 min

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$ :

(a) $2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m$ at $500 K$

(b) $C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m$ at $1073 K$

Text solutionVerified

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Find out the value of Kc​ for each of the following equilibria from the value of Kp​:(a) 2NOCl(g)​⇌2NO(g)​+Cl2(g)​ ; Kp​=1.8×10−2atm at 500 K(b) CaCO3(s)​⇌CaO(s)​+CO2(g)​ ; Kp​=167 atm at 1073 K

Text solutionVerified

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Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$ :

(a) $2 NOC l_{(g)} ⇌ 2 N O_{(g)} + C l_{2 (g)}; K_{p} = 1.8 \times 1 0^{- 2} a t m$ at $500 K$

(b) $C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}; K_{p} = 167 a t m$ at $1073 K$