(D) For reaction $(i)$: $N_2 + 2O_2 \rightleftharpoons 2NO_2$ with equilibrium constant $K_1$.For reaction $(ii)$: $2NO_2 \rightleftharpoons N_2 + 2O_

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(D) For reaction $(i)$: $N_2 + 2O_2 \rightleftharpoons 2NO_2$ with equilibrium constant $K_1$.For reaction $(ii)$: $2NO_2 \rightleftharpoons N_2 + 2O_2$,which is the reverse of $(i)$,so $K_2 = 1/K_1$.For reaction $(iii)$: $NO_2 \rightleftharpoons 1/2 N_2 + O_2$,which is half of reaction $(ii)$,so $K_3 = (K_2)^{1/2} = \sqrt{K_2}$.From $K_2 = 1/K_1$,we get $K_1 = 1/K_2$.From $K_3 = \sqrt{K_2}$,we get $K_3^2 = K_2$,so $K_2 = K_3^2$.Substituting $K_2$ in $K_1 = 1/K_2$,we get $K_1 = 1/K_3^2$.

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

Medium

The equilibrium constants for the reactions $(i)$,$(ii)$,and $(iii)$ are $K_1$,$K_2$,and $K_3$ respectively. Which of the following is the correct relationship?
$(i)$ $N_2 + 2O_2 \rightleftharpoons 2NO_2$
$(ii)$ $2NO_2 \rightleftharpoons N_2 + 2O_2$
$(iii)$ $NO_2 \rightleftharpoons 1/2 N_2 + O_2$

A
$K_1 = \sqrt{K_2} = K_3$
B
$K_1 = 1/K_2 = 1/K_3$
C
$K_1 = K_2^2 = K_3$
D
$K_1 = 1/K_2 = 1/(K_3)^2$

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6-1.Equilibrium (Chemical Equilibrium)

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Law of equilibrium and Equilibrium constant

The figure shows the change in concentration of species $A$ and $B$ as a function of time. The equilibrium constant $K_C$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)}$ is

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$3 O_{2(g)} \rightleftharpoons 2 O_{3(g)}$
For the above reaction at $298 \ K$,$K_c$ is found to be $3.0 \times 10^{-59}$. If the concentration of $O_2$ at equilibrium is $0.040 \ M$,then the concentration of $O_3$ in $M$ is ...... .

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For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,which of the following expressions for the equilibrium constant $K_p$ is correct?

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Consider the following gaseous equilibria with equilibrium constants $K_{1}$ and $K_{2}$ respectively:
$SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$
$2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)}$
The equilibrium constants are related as:

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$4$ moles of $A$ are mixed with $4$ moles of $B$. At equilibrium for the reaction $A + B \rightleftharpoons C + D$,$2$ moles of $C$ and $D$ are formed. The equilibrium constant for the reaction will be

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The equilibrium constants for the reactions $(i)$,$(ii)$,and $(iii)$ are $K_1$,$K_2$,and $K_3$ respectively. Which of the following is the correct relationship?$(i)$ $N_2 + 2O_2 \rightleftharpoons 2NO_2$$(ii)$ $2NO_2 \rightleftharpoons N_2 + 2O_2$$(iii)$ $NO_2 \rightleftharpoons 1/2 N_2 + O_2$

Similar Questions

The figure shows the change in concentration of species $A$ and $B$ as a function of time. The equilibrium constant $K_C$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)}$ is

$3 O_{2(g)} \rightleftharpoons 2 O_{3(g)}$For the above reaction at $298 \ K$,$K_c$ is found to be $3.0 \times 10^{-59}$. If the concentration of $O_2$ at equilibrium is $0.040 \ M$,then the concentration of $O_3$ in $M$ is ...... .

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Consider the following gaseous equilibria with equilibrium constants $K_{1}$ and $K_{2}$ respectively: $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$ $2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)}$ The equilibrium constants are related as:

$4$ moles of $A$ are mixed with $4$ moles of $B$. At equilibrium for the reaction $A + B \rightleftharpoons C + D$,$2$ moles of $C$ and $D$ are formed. The equilibrium constant for the reaction will be

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The equilibrium constants for the reactions $(i)$,$(ii)$,and $(iii)$ are $K_1$,$K_2$,and $K_3$ respectively. Which of the following is the correct relationship?
$(i)$ $N_2 + 2O_2 \rightleftharpoons 2NO_2$
$(ii)$ $2NO_2 \rightleftharpoons N_2 + 2O_2$
$(iii)$ $NO_2 \rightleftharpoons 1/2 N_2 + O_2$

$3 O_{2(g)} \rightleftharpoons 2 O_{3(g)}$
For the above reaction at $298 \ K$,$K_c$ is found to be $3.0 \times 10^{-59}$. If the concentration of $O_2$ at equilibrium is $0.040 \ M$,then the concentration of $O_3$ in $M$ is ...... .

Consider the following gaseous equilibria with equilibrium constants $K_{1}$ and $K_{2}$ respectively:
$SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$
$2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)}$
The equilibrium constants are related as: