(B) The given reactions are:$(i) \ S(s) + S^{2-}(aq) \rightleftharpoons S_2^{2-}(aq) \quad K_1 = 1.7$$(ii) \ 2S(s) + S^{2-}(aq) \rightleftharpoons S_3

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(B) The given reactions are:$(i) \ S(s) + S^{2-}(aq) \rightleftharpoons S_2^{2-}(aq) \quad K_1 = 1.7$$(ii) \ 2S(s) + S^{2-}(aq) \rightleftharpoons S_3^{2-}(aq) \quad K_2 = 5.3$We need to find the equilibrium constant $K$ for the reaction:$(iii) \ S(s) + S_2^{2-}(aq) \rightleftharpoons S_3^{2-}(aq)$By observing the reactions,we can see that $(iii) = (ii) - (i)$.Therefore,the equilibrium constant $K$ is given by:$K = \frac{K_2}{K_1} = \frac{5.3}{1.7} \approx 3.11$

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

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In an alkaline medium,the sulfide ion reacts with solid sulfur to form polysulfide ions. The equilibrium constants for the formation of $S_2^{2-}$ and $S_3^{2-}$ from $S$ and $S^{2-}$ ions are $1.7$ and $5.3$,respectively. The equilibrium constant for the formation of $S_3^{2-}$ from $S_2^{2-}$ and $S$ will be .........

A
$1.33$
B
$3.11$
C
$4.21$
D
$1.63$

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6-1.Equilibrium (Chemical Equilibrium)

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

$2SO_2 + O_2 \to$ product. If the pressure of the reaction increases $3$ times, then the rate will be (in $\times$)?

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At $717 \ K$,$3.2 \ mol$ of $HI$ is heated in a closed tube. $20\%$ of $HI$ decomposes at equilibrium according to the reaction $2HI_{(g)} \rightleftharpoons H_{2_{(g)}} + I_{2_{(g)}}$. Find $K_c$ and the moles of $HI$,$H_2$,and $I_2$ at equilibrium.

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Which of the following statements is false?

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At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

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$CH_3COCH_{3(g)} \rightleftharpoons C_2H_{6(g)} + CO_{(g)}$. The initial pressure of $CH_3COCH_3$ is $100 \ mm$. When equilibrium is set up,the mole fraction of $CO_{(g)}$ is $\frac{1}{4}$. Hence,the partial pressure of $CO$ is:

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$2SO_2 + O_2 \to$ product. If the pressure of the reaction increases $3$ times, then the rate will be (in $\times$)?

At $717 \ K$,$3.2 \ mol$ of $HI$ is heated in a closed tube. $20\%$ of $HI$ decomposes at equilibrium according to the reaction $2HI_{(g)} \rightleftharpoons H_{2_{(g)}} + I_{2_{(g)}}$. Find $K_c$ and the moles of $HI$,$H_2$,and $I_2$ at equilibrium.

Which of the following statements is false?

At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.$(i)$ Find $K_p$.$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

$CH_3COCH_{3(g)} \rightleftharpoons C_2H_{6(g)} + CO_{(g)}$. The initial pressure of $CH_3COCH_3$ is $100 \ mm$. When equilibrium is set up,the mole fraction of $CO_{(g)}$ is $\frac{1}{4}$. Hence,the partial pressure of $CO$ is:

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At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?