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: Objective Chemistry for NEET
Uploaded: 2021-10-14T06:24:11-08:00
Duration: 1 min 4 s
Channel: Narayan Hari
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, I can write the value of KC1 is equal to S -O2 -O2 to the power 1 by 2 by S -O3

Question

The equilibrium constant for the reaction: $\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})$ is $\mathrm{K}_{\mathrm{c}}=4.9 \times 10^{-2}$. The value of $\mathrm{K}_{c}$ 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:
$\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})$
is $\mathrm{K}_{\mathrm{c}}=4.9 \times 10^{-2}$. The value of $\mathrm{K}_{c}$ 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) $4.9 \times 10^{-2}$

Objective Chemistry for NEET

A.K. Singhal, U. K.… 1st Edition

Chapter 7, Problem 57

Instant Answer

Solved by Expert Narayan Hari

10/14/2021

Step 1

9 \times 10^{-2}$. Show more…

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The equilibrium constant for the reaction: $\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})$ is $\mathrm{K}_{\mathrm{c}}=4.9 \times 10^{-2}$. The value of $\mathrm{K}_{c}$ 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) $4.9 \times 10^{-2}$

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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.

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