The equilibrium constant for the reaction, SO3( g) ⇌SO2( g)+1 / 2 O2( g) is Kc=4.9 ×10^-2 . The

Name: Problem 57, Chapter 7: A Complete Resource Book in Chemistry for JEE Main
Uploaded: 2021-10-13T07:30:55-08:00
Duration: 3 min 16 s
Channel: Preeti Kumari
Description: The equilibrium constant for the reaction, SO3( g) ⇌SO2( g)+1 / 2 O2( g) is Kc=4.9 ×10^-2 . The value of Kc for the reaction 2 SO2( g)+O2( g) ⇌2 SO3( g) will be (a) 416 (b) 2.40 ×10^-3 (c) 9.8 ×10^-2 (d) 4.9 ×10^-2

step 1 In this problem, we have given a reaction, SO3 decomposes reversibly to give SO2 and half mole o

Question

The equilibrium constant for the reaction, $\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g})$ is $K_{c}=4.9 \times 10^{-2} .$ The value of $K_{c}$ for the reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$ will be (a) 416 (b) $2.40 \times 10^{-3}$ (c) $9.8 \times 10^{-2}$ (d) $4.9 \times 10^{-2}$

   The equilibrium constant for the reaction, $\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g})$
is $K_{c}=4.9 \times 10^{-2} .$ The value of $K_{c}$ for the reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$ will be
(a) 416
(b) $2.40 \times 10^{-3}$
(c) $9.8 \times 10^{-2}$
(d) $4.9 \times 10^{-2}$

A Complete Resource Book in Chemistry for JEE Main

A.K. Singhal 3rd Edition

Chapter 7, Problem 57

Instant Answer

Solved by Expert Preeti Kumari

10/13/2021

Step 1

9 \times 10^{-2}$. The expression for this equilibrium constant can be written as: \[K_{c} = \frac{[\mathrm{SO}_{2}][\mathrm{O}_{2}]^{1/2}}{[\mathrm{SO}_{3}]} = 4.9 \times 10^{-2}\] Show more…

Show all steps

Thanks for your feedback!

The equilibrium constant for the reaction, $\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g})$ is $K_{c}=4.9 \times 10^{-2} .$ The value of $K_{c}$ for the reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$ will be (a) 416 (b) $2.40 \times 10^{-3}$ (c) $9.8 \times 10^{-2}$ (d) $4.9 \times 10^{-2}$

Play audio

Feedback

Preeti Kumari and 93 other subject Chemistry 102 educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Equilibrium Constant (Kc)

The equilibrium constant expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. Its value is specific to the reaction at a given temperature and is used to predict the extent of the reaction under equilibrium conditions.

Reaction Stoichiometry and Its Effect on Kc

The equilibrium constant is dependent on the stoichiometry of the reaction. When the reaction is reversed, the equilibrium constant becomes the reciprocal of the original. Additionally, when the coefficients of a balanced equation are multiplied by a factor, the equilibrium constant is raised to that power, reflecting the change in the reaction's stoichiometry.

Please give Ace some feedback