(C) For the first reaction: $K_1 = \frac{[SO_3]}{[SO_2][O_2]^{1/2}}$For the second reaction: $K_2 = \frac{[SO_2]^2[O_2]}{[SO_3]^2}$Comparing the two e

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(C) For the first reaction: $K_1 = \frac{[SO_3]}{[SO_2][O_2]^{1/2}}$For the second reaction: $K_2 = \frac{[SO_2]^2[O_2]}{[SO_3]^2}$Comparing the two expressions,we can see that $K_2 = \left( \frac{1}{K_1} \right)^2 = \frac{1}{K_1^2}$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Law of equilibrium and Equilibrium constant

Easy

For the reactions $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,if the equilibrium constants at $298 \ K$ are $K_1$ and $K_2$ respectively,then the correct relationship between them is .......

A
$K_1 = K_2$
B
$K_2 = K_1^2$
C
$K_2 = \frac{1}{K_1^2}$
D
$K_2 = \frac{1}{K_1}$

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Class 11

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Chapter

6-1.Equilibrium (Chemical Equilibrium)

Subtopic

Law of equilibrium and Equilibrium constant

The equilibrium constant $K_{c}$ at $298 \ K$ for the reaction $A + B \rightleftharpoons C + D$ is $100$. Starting with an equimolar solution with concentrations of $A$,$B$,$C$ and $D$ all equal to $1 \ M$,the equilibrium concentration of $D$ is $....... \times 10^{-2} \ M$. (Nearest integer)

MediumJEE MAIN 2021

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On a given condition,the equilibrium concentrations of $HI$,$H_2$,and $I_2$ are $0.80 \ mol/L$,$0.10 \ mol/L$,and $0.10 \ mol/L$ respectively. The equilibrium constant for the reaction $H_2 + I_2 \rightleftharpoons 2HI$ will be:

Difficult

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$5 \ moles$ each of $H_2$ and $I_2$ were heated in a sealed $10 \ L$ vessel. At equilibrium,$2 \ moles$ of $HI$ were found. The equilibrium constant for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is:

Medium

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The equilibrium constant $K_C$ of the reaction,$2 A \rightleftharpoons B + C$ is $0.5$ at $25^{\circ} C$. The reaction will proceed in the backward direction,when concentrations $[A], [B]$ and $[C]$ are,respectively:

MediumKVPY 2014

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$4.5 \text{ moles}$ each of hydrogen and iodine is heated in a sealed $10 \text{ litre}$ vessel. At equilibrium,$3 \text{ moles}$ of $HI$ were found. The equilibrium constant for $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is .......

EasyJEE MAIN 2023

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For the reactions $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,if the equilibrium constants at $298 \ K$ are $K_1$ and $K_2$ respectively,then the correct relationship between them is .......

Similar Questions

The equilibrium constant $K_{c}$ at $298 \ K$ for the reaction $A + B \rightleftharpoons C + D$ is $100$. Starting with an equimolar solution with concentrations of $A$,$B$,$C$ and $D$ all equal to $1 \ M$,the equilibrium concentration of $D$ is $....... \times 10^{-2} \ M$. (Nearest integer)

On a given condition,the equilibrium concentrations of $HI$,$H_2$,and $I_2$ are $0.80 \ mol/L$,$0.10 \ mol/L$,and $0.10 \ mol/L$ respectively. The equilibrium constant for the reaction $H_2 + I_2 \rightleftharpoons 2HI$ will be:

$5 \ moles$ each of $H_2$ and $I_2$ were heated in a sealed $10 \ L$ vessel. At equilibrium,$2 \ moles$ of $HI$ were found. The equilibrium constant for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is:

The equilibrium constant $K_C$ of the reaction,$2 A \rightleftharpoons B + C$ is $0.5$ at $25^{\circ} C$. The reaction will proceed in the backward direction,when concentrations $[A], [B]$ and $[C]$ are,respectively:

$4.5 \text{ moles}$ each of hydrogen and iodine is heated in a sealed $10 \text{ litre}$ vessel. At equilibrium,$3 \text{ moles}$ of $HI$ were found. The equilibrium constant for $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is .......

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