(B) The target reaction is: $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$Given reactions:$(i) \ S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)

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(B) The target reaction is: $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$Given reactions:$(i) \ S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$$(ii) \ 2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$To obtain the target reaction,we perform the operation: $(ii) - 2 \times (i)$:$2SO_{3(g)} - 2SO_{2(g)} = (2S + 3O_2) - 2(S + O_2) = O_{2(g)}$Thus,the equilibrium constant $K_{eq}$ is given by:$K_{eq} = \frac{K_2}{(K_1)^2}$$K_{eq} = \frac{10^{129}}{(10^{52})^2} = \frac{10^{129}}{10^{104}} = 10^{25}$

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Medium

For the following reactions,equilibrium constants are given:
$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$
$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$
The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is:

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A
$10^{77}$
B
$10^{25}$
C
$10^{181}$
D
$10^{154}$

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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At $T$ $(K)$,$K_c$ for the dissociation of $PCl_5$ is $2 \times 10^{-2} \ mol \ L^{-1}$. The number of moles of $PCl_5$ that must be taken in a $1.0 \ L$ flask at the same temperature to get $0.2 \ mol$ of chlorine at equilibrium is:

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For the following reactions,equilibrium constants are given:$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is:

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For a reaction $2 A \rightleftharpoons B + C$,$K_c$ is $2 \times 10^{-3}$. At a given time,the reaction mixture has $[A] = [B] = [C] = 3 \times 10^{-4} \ M$. Which of the following options is correct?

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,what is the relationship between $\Delta H$ and $\Delta E$?

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At $T$ $(K)$,$K_c$ for the dissociation of $PCl_5$ is $2 \times 10^{-2} \ mol \ L^{-1}$. The number of moles of $PCl_5$ that must be taken in a $1.0 \ L$ flask at the same temperature to get $0.2 \ mol$ of chlorine at equilibrium is:

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For the following reactions,equilibrium constants are given:
$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$
$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$
The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is: