For the reaction, 2SO2(g)+O2(g)⟶2SO3(g), ΔH=−57.2 kJ mol−1 and Kc=1.7×1016. Which of the following statement is incorrect?

Name: Video answer for For the reaction, 2SO2(g)+O2(g)⟶2SO3(g), ΔH=−57.2 kJ mol−1 and Kc=1.7×1016. Which of the following statement is incorrect?
Uploaded: 2023-03-01T10:11:15.000Z
Duration: 15 min
Description: For the reaction, 2SO2(g)+O2(g)⟶2SO3(g), ΔH=−57.2 kJ mol−1 and Kc=1.7×1016. Which of the following statement is incorrect?

Applications of equilibrium constant

For the reaction, 2 {SO}_{2}(g)+{O}_{2}(g) 2 {SO}_{3}(g), H=

Question

Medium

Solving time: 3 mins

For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g),$ $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16} .$ Which of the following statement is incorrect?

The equilibrium constant decreases as the temperature increases

The addition of inert gas at constant volume will not affect the equilibrium constant

The equilibrium will shift in forward direction as the pressure increases

The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required

Views: 5,599 students

Updated on: Mar 1, 2023

Book:

Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

Exam:

JEE Mains 2019

Text solutionVerified

The explanation of given statements are as follows: (a) For the given equilibrium,

Δ H

is negative, so the equilibrium constant will decrease with increase in temperature and the equilibrium will shift in the backward direction. Thus, statement (a) is correct. (b) When inert gas is added at constant volume and constant temperature, an equilibrium remains undisturbed. Thus, statement (b) is correct. (c) For the equilibrium,

Δ n_{g} = 2 - (2 + 1) = - 1

, i.e.

(-

)

So, increase in pressure will shift the equilibrium in the forward direction. Thus, statement (c) is correct. (d) The reaction takes place in the presence of a catalyst which is

V_{2} O_{5} (s)

in contact process or

NO (g)

in chamber process. Thus, statement (d) is incorrect.

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Elijah Discussed

For the reaction,

2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g),

Δ H = - 57.2 kJ mol^{- 1}

and

K_{c} = 1.7 \times 1 0^{16} .

Which of the following statement is incorrect?

7 mins ago

Discuss this question LIVE

7 mins ago

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Question Text	For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g),$ $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16} .$ Which of the following statement is incorrect?
Updated On	Mar 1, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	200
Avg. Video Duration	15 min

For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g),$ $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16} .$ Which of the following statement is incorrect?

Text solutionVerified

Video solutions (1)

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For the reaction, 2SO2​(g)+O2​(g)⟶2SO3​(g), ΔH=−57.2 kJ mol−1 and Kc​=1.7×1016. Which of the following statement is incorrect?

Text solutionVerified

Video solutions (1)

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Practice questions from Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

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For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g),$ $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16} .$ Which of the following statement is incorrect?