(C) For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,the equilibrium constant is $K = 278$.Reversing the reaction gives $2SO_{3(

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(C) For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,the equilibrium constant is $K = 278$.Reversing the reaction gives $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,for which the equilibrium constant is $K' = \frac{1}{K} = \frac{1}{278}$.Dividing the stoichiometric coefficients of the reversed reaction by $2$ gives the target reaction: $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$.The equilibrium constant for this reaction is $K'' = \sqrt{K'} = \sqrt{\frac{1}{278}} \approx 0.0599 \approx 6.0 \times 10^{-2}$.

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

Difficult

Given that the equilibrium constant for the reaction,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ has a value of $278$ at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature? $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$

AIPMT 2012 All AIPMT

A
$1.8 \times 10^{-3}$
B
$3.6 \times 10^{-3}$
C
$6.0 \times 10^{-2}$
D
$1.3 \times 10^{-5}$

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6-1.Equilibrium (Chemical Equilibrium)

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Law of equilibrium and Equilibrium constant

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AIPMT 2012 Paper All AIPMT years →

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DifficultIIT 2001

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Medium

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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 .......

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For the reaction $x \rightleftharpoons y$,which of the following factors will affect the value of $[\text{Product}] / [\text{Reactant}]^{-1}$ at equilibrium?

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At constant temperature,the equilibrium constant $(K_p)$ for the decomposition reaction $N_2O_4 \rightleftharpoons 2NO_2$ is expressed by $K_p = \frac{4x^2P}{1 - x^2}$,where $P = \text{pressure}$,$x = \text{extent of decomposition}$. Which one of the following statements is true?

The following concentrations were obtained for the formation of $NH_{3}$ from $N_{2}$ and $H_{2}$ at equilibrium at $500\, K$: $[N_{2}] = 1.5 \times 10^{-2}\, M$,$[H_{2}] = 3.0 \times 10^{-2}\, M$ and $[NH_{3}] = 1.2 \times 10^{-2}\, M$. Calculate the equilibrium constant.

At a definite temperature,the equilibrium constant $K_{c}$ is given by the following equation: $K_{c} = \frac{[I_{2}][H_{5}IO_{6}]^{5}}{[IO_{3}^{-}]^{7}[H_{2}O]^{9}[H^{+}]^{7}}$. Write the balanced chemical equilibrium equation.

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 .......

For the reaction $x \rightleftharpoons y$,which of the following factors will affect the value of $[\text{Product}] / [\text{Reactant}]^{-1}$ at equilibrium?

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